Ideal Gas Law

Key Questions

• What are the limitations of the ideal gas law?

  Answer:

  The ideal gas law makes some assumptions about gases that are not necessarily true. This means that the ideal gas law has some limitations.

  Explanation:

  For example, the ideal gas law makes an assumption that gas particles have no volume and are not attracted to each other.

  Here's why the idea gas law has limitations.

  1. Imagine that you condense an ideal gas. Since the particles of an ideal gas have no volume, a gas should be able to be condensed to a volume of zero. Reality check: Real gas particles occupy space. A gas will be condensed to form a liquid which has volume. The gas law no longer applies because the substance is no longer a gas!

  2. Same scenario. We assume that gas particles are not attracted to each other. Reality check: Real gas particles are attracted to each other. As kinetic energy decreases as a gas is cooled, the particles will eventually move slowly enough that there attractive forces cause them to condense. The gas law no longer applies because the substance is no longer a gas!

  mrpauller.weebly.com · 19 · Jun 27 2014

• How do you find the ideal gas constant?
• How do you solve ideal gas law problems?
• How do you know which ideal gas constant to use?
• What is the ideal gas constant for butane?
• Why is ideal gas law in kelvin?
• Why is the ideal gas constant important?
• What is the di-electric constant?
• What volume (L) will 0.20 mol HI occupy at 300 K and 100.0 kPa? R = 8.314 kPa L / (K mol) = 0.08205 atm L / (mol K)?
• How do you calculate the molar mass of a gas?
• When should I use the ideal gas law and not the combined gas law?
• What does the ideal gas law allow a scientist to calculate that the other gas laws do not?
• Why is ideal gas law important?
• How do you calculate the density of a gas with temperature change?
• What form of the ideal gas law would you use to calculate the temperature of a gas?
• What is the density of hydrogen gas using the ideal gas law?
• How do you solve Ideal Gas Law problems?
• If an ideal gas occupies 27.5 ml at 760 torr and 23 °C then, what volume would the same gas occupy at standard conditions?
• What is the relationship between the ideal gas law and the Avogadro's law?
• What is the ideal gas law constant?
• What units should I use in the ideal gas law equation?
• What is the molar form of the ideal gas law?
• What is n in the equation of the ideal gas law?
• What is R in the mathematical expression of the ideal gas law?
• What is the relationship between the ideal gas law and the kinetic theory?
• What is the equation of the ideal gas law?
• What are the limitations of the ideal gas law?
• How does the ideal gas law differ from the combined gas law?
• What is the relationship between the combined gas law and the ideal gas law?
• Can the ideal gas law be applied to liquids?
• How does the ideal gas law confirm the laws of Boyle and Charles?
• Question #c1c9e
• Question #7152a
• Question #fbab1
• Question #b0220
• We have a lab assignment that we haven't had a lecture on yet. It's the Pv=nRT. I had to graph 50 plus atm measurements & K temps on Excel. We are supposed to answer "# of moles of the gas in the 250mL sealed flask." I do not know where to go next?
• Question #ba20f
• Question #37e6a
• Question #6d7e7
• Question #6715e
• Question #32af4
• Question #34f5b
• Question #6e7c9
• At a pressure of #"185 mmHg"# and a temperature of #55^@"C"#, what volume would #2.55xx10^28# molecules of nitrogen gas occupy?
• Question #00893
• Question #dd886
• What is the mass in kg of butane in a #"20 L"# cylinder with a pressure of #"0.963 atm"# and a temperature of #27^@"C"#?
• Question #4760a
• Question #de464
• 2 C8H18(l) + 25 O2(g) ----> 16 CO2(g) + 18 H2O(g) If 4.00 moles of gasoline are burned, what volume of oxygen is needed if the pressure is 0.953 atm, and the temperature is 35.0°C?
• 2 C8H18(l) + 25 O2(g) #-># 16 CO2(g) + 18 H2O(g) If you burned one gallon of gas (C8H18) (approximately 4000 grams), how many liters of carbon dioxide would be produced at a temperature of 21.0°C and a pressure of 1.00 atm?
• 2 Cl2(g) + C2H2(g) ‡ C2H2Cl4(l) How many liters of chlorine will be needed to make 75.0 grams of C2H2Cl4? Pressure: 1 atm Temperature: 298K
• Question #2849f
• Question #ebbe0
• How many moles of ammonia are there in a 5.00 L cylinder if they exert a pressure of 8.65 atm at 18.0 Celsius?
• At 18.0 Celsius and 765 torr, 2.29 dm^3 of a gas weigh 3.71 g. How to calculate the approximate molar mass, in g/mol, of the gas?
• How many grammes of zinc metal are required to produce 10.0 litres of hydrogen gas, at 25 Celsius and 1.00 atm pressure, by reaction with excess hydrochloric acid? Zn (s) + 2HCl (aq)  ZnCl2 (aq) + H2 (g) ?
• Octane (C8H18, 114.23 g/mol). The density of octane vapour 125.0 Celsius and 720.0 torr is ? and what would be the volume be if it was 2.00 moles ?
• Question #52ffd
• Question #1b0c9
• Question #7d3c8
• Question #fb71c
• 0.465 g sample of an unknown compound occupies 245 mL at 298K and 1.22 atm. What is the molar mass of the unknown compound?
• How many milliters of oxygen are required to react completely with 175 mL of C4H10 if the volumes of both gases are measured at the same temperature and pressure? The reaction is 2C4H(g) + 13O2(g) --> 8CO2(g) +10H2O(g)
• Question #13daf
• What pressure (in torr) is exerted by 10.0 g of O2 in a 2.50 L container at a temperature of 27 degree C?
• Propylene, C3H6, reacts with hydrogen under pressure to give propane, C3H8: C3H6(g) + H2(g) -----> C3H8(g) How many liters of hydrogen ( at 740 torr and 24 degree C) react with 18.0 g of propylene?
• The pressure in a 5.75 L container of 48.0 g of bromine gas at 100.0°C is ....... What is the pressure in atm?
• What volume in liters does 0.136 g of O2 occupy at 20.0 degree C and 748 torr?
• Question #c4095
• Question #c7d69
• Question #9bd40
• Question #7a15c
• Question #d0d53
• Question #b27c0
• Question #2ed61
• Question #7a48b
• Question #cee00
• Question #41adf
• Question #2e2b3
• In this reaction, 4.58L of #O_2# were formed at 745 mmHg and 308K. How many grams of #Ag_2O# decomposed? #2Ag_2O_((s)) -> 4Ag_((s)) + O_(2(g))#
• Question #e95a0
• Question #5d74d
• Question #11c36
• Question #a334f
• Question #e66a1
• Question #75041
• Considering the ideal gas law PV=nRT, what is P directly proportional to what variable?
• Question #ef6c6
• Question #20ca9
• Question #a5357
• Question #ef2ef
• Question #e3578
• 0.4g of a gas has a volume of 227cm^3 at 27°C and at a pressure of 100kPa. Calculate the relative molecular mass of the gas (R=8.31 J/kmol)?
• Question #51550
• Question #1499b
• Question #24fe2
• Question #4ceaa
• What units are used in the equation pv=nrt?
• How would you solve for n in PV=nRT?
• In the equation pv=nrt, how would you solve for v?
• Suppose that 7.47 x 10^-3mol of hydrogen gas occupies a 335 mL container at -91°C what is the pressure (in torr)? i know the answer is 253 .. but idk how to work it? someone please help me?
• A sample of gas occupies a volume of 272 mL at a pressure of .999 atm and a temp of 357K. If the sample weighs 1.03 g, what is the molecular weight of the gas?
• How would you solve the equation PV = nRT for R?
• What does the R in PV=nRT represent?
• Considering the ideal gas law PV = nRT, what is P directly proportional to?
• How would you derive the ideal gas law PV= nRT using Avogadros law, Boyles law, and Charles law?
• In the ideal gas law, what would you use for R when P is in Pascals?
• Given a jar of gas (fixed volume and pressure) at 273.15K, the temperature is lowered to 0K, what happens to the volume?
• How would you derive the ideal gas equation?
• Given that 6.6 moles of carbon monoxide gas are present in a 43.3L container, what is the pressure of the gas (in atm) if the temperature is 84°C?
• Question #5f2c7
• An experiment shows that a 245mL gas sample has a mass of 0.436g at a pressure of 757 mmHg and a temperature of 29C. What is the molar mass of the gas?
• If 2.30 g occupies 0.870 L at 690 torr and 37 degrees C. How would you calculate the molar mass?
• An imaginary ideal gas has a density of 3 g/L at STP. What is the molar mas of this gas?
• What is the mass of neon that exerts a pressure of 720 mmHg with a temperature of -15.0°C, when the volume of the container is 760 mL?
• How would you find the volume of 7 moles of CH4 at standard temperature and pressure?
• When would you use the combined gas law as opposed to the ideal gas law?
• What is the mass of a sample of CO2 if it is held at 24 degrees C, 0.544 atm in a 3.00L flask?
• Who discovered the Ideal Gas Law?
• What does the constant R in the Ideal Gas Law mean?
• The air inside a beach ball is at a temp of 25 degrees Celsius, and a pressure of 1.0 atm. If the ball contains .85 mol of air what is the volume?
• Each molecule of hemoglobin combines with four molecules of O2. If 1.00g hemoglobin combines with 1.60mL O2 at 37oC and 99.0 kPa, what is the molar mass of hemoglobin?
• A gas sitting in a 5L container at 12 degrees celcius at 3atm, how many moles do you have?
• When using the ideal gas constant value, R = 0.0821, in an ideal gas law calculation, what are the units of volume?
• How would you find the number of grams of CO2 that exert a pressure of 785 torrs at a volume of 32.5 L and a temperature of 32 degrees C?
• Under what conditions is a gas closest to properties of an ideal gas?
• What does the ideal gas law allow a scientist to calculate that the other gas laws do not?
• In the equation PV=nRT, what does the R and n stand for?
• How many grams of CO(g) are there in 745 ml of the gas at 1.03 atm and 36 degrees celsius ?
• How would you determine the volume that 1 mol of a gas at 0°C and 1 atm occupies?
• How would you calculate the volume of 3.03 g of H2(g) at a pressure of 560 torr and temp of 139 k?
• Question #0ea44
• Question #75905
• A gas occupies #"67. cm"^3# at #9.38 × 10^4color(white)(l)"Pa"# and 22 °C. What is its volume at #10.6 × 10^5color(white)(l)"Pa"# and 29 °C?
• Question #9008a
• How many liters would 14.0 grams of chlorine gas occupy at 300.0 K and 1.51 atm?
• I've found the number of moles of each gas (H2 and H2O) using PV = nRT. Now. I need to find the theoretical yield of H at STP. Can you refresh my memory on how to do that? Is it different with gases?
• A sample of #O_2# gas is stored at 30.0 °C and 755 torr. If the volume was 125mL, how much did the oxygen weigh?
• Question #0462f
• A 3.0 mol gas sample occupies 6.0 liters at 25 °C. What is the pressure of the gas in kPa’s?
• Question #79f4c
• A #89.9# g sample of dinitrogen monoxide is confined in a #3.65#-L vessel. What is the pressure (in atm) at #110# degrees Celsius?
• How many molecules of #CO_2# gas at 713 mmHg and 56.7°C are present in 10.5 L?
• Question #8b6ce
• Question #bd933
• Question #71b77
• How many kilograms of #O_2# gas are needed to give an oxygen pressure of 3.48 atm at 22°C?
• Question #69194
• Question #60299
• What volume does 0.0250 mole #H_2# occupy at 0.821 atm pressure and 300 K?
• What does the ideal gas law allow a scientist to calculate that the other gas laws do not?
• Who discovered the Ideal Gas Law?
• If a 0.614 g sample of a gas maintains a pressure of 238 mm Hg when contained in a 1.0L flask at 0.0°C, what is the gases molecular weight?
• What is the volume occupied by 10.8 g of argon gas at a pressure of 1.30 atm and a temperature of 408 K?
• What is the mole fraction of #NO# in a 55.0 L gas cylinder at 30.0°C which comes from a mixture of #N_2# and #NO# if you have 3.238 mol of #N_2# and the gas cylinder has a total pressure of 2.14 atm?
• What is the pressure in 2 L balloon which contains 5 moles of gas at a temperature of 250 K?
• What is the temperature of 2.0 moles of a gas occupying a volume of 5.0 L at 2.46 atm?
• What is the volume occupied by 25.2 g of #CO_2# at .84 atm and 25°C?
• What is the molar mass of a gas if a 0.950 gram sample of it occupies 232 mL at 95 °C and 0.985 atm?
• Question #73fe8
• A gaseous hydrocarbon collected over water at a temperature of 21° C and a barometric pressure of 753 torr occupied a volume of 48.1 mL. The hydrocarbon in this volume weighs 0.1133 g. What is the molecular mass of the hydrocarbon?
• The density of air #20# #km# above Earths surface is #92# #g##/##m^3.# The pressure of the atmosphere is #42# #mm# #Hg#, and the temperature is #-63# #°C#. What is the average molar mass of the atmosphere at this altitude?
• You heat 0.158g of a white, solid carbonate of a Group 2 metal and find that the evolved #CO_2# has a pressure of 69.8 mmHg In a 285ml flask at 25°C .What is the molar mass of the metal carbonate?
• If a 0.050g sample of the boron hydride burns completely in #O_2#, what will be the pressure of the gaseous water In a 4.25-L flask at 30.0°C?
• What is the density of acetylene gas measured at pressure of 0.75 atm and temperature of 250°C?
• You heat 0.158g of a white, solid carbonate of a Group 2 metal and find that the evolved #CO_2# has a pressure of 69.8mmHg in a 285ml flask at 25°C. What is the molar mass of the metal carbonate?
• The atmospheric pressure at the summit of Mt. Everest is 255 torr. The percentage of #O_2# and #N_2# is 20% and 79%, respectively. How many #N_2# and #O_2# molecules are there in a volume of 10.0L at 12°C?
• What is the density of krypton gas at STP?
• Question #4ea7f
• What is the volume of #H_2# generated by reacting 4.33g of #Zn# with excess #H_2SO_4# at 38°C and 760 torr?
• The hydrogen chloride gas used to make polyvinyl chloride plastic is made by reacting hydrogen gas with chlorine gas. What volume of HCL at 105 kPa and 296 K can be formed from 1150 #m^3# of #H_2# at STP?
• Question #f784e
• Question #423de
• An ideal gas has a volume of 2.28 L at 279 K and 1.07 atm. What is the pressure when the volume is 1.03 L and the temperature is 307 K?
• Question #7db3d
• Question #71e1b
• What is the temperature in Celsius inside a sealed 10.0 L flask which contains 14.2 g of nitrogen gas at 2.0 atm?
• A gas takes up a volume of 19.5 liters, has a pressure of 2.9 atm, and a temperature of 5.5°C. If I raise the temperature to 65°C and lower the pressure to 1.5 atm, what is the new volume of the gas?
• What is the volume of 2.0 moles of an ideal gas at 290 K and 2.8 atm?
• A 21-liter cylinder contains 1.5 moles of an ideal gas at 311 K. What is the pressure of the gas?
• Question #9b73a
• Question #eac5b
• Question #eac7c
• How many moles of #CO_2# (g) are in a 5.6 L sample of #CO_2# measured at STP?
• How many moles are in a gas in 890mL at 21 °C and 750 mmHg?
• A technician is designing an airbag for a new model car. She wants to use 72.0g of sodium azide (#NaN_3#) to inflate the bag at 22.0°C and 1.00 atm. What is the maximum volume of the airbag under these conditions?
• A 283.3-g sample of #X_2(g)# has a volume of 30 L at 3.2 atm and 27°C. What is element #X#?
• What volume will 12.0 g of oxygen gas (#O_2#) occupy at 25°C and a pressure of 52.7 kPa?
• A gas canister can tolerate internal pressures up to 210 atmospheres. If a 2.0 L canister holding 3.5 moles of gas is heated to 1350° C, will the canister explode?
• If 5.0 moles of #O_2# and 3.0 moles of #N_2# are placed in a 30.0 L tank at a temperature of 25°C, what will the pressure of the resulting mixture of gases be?
• Question #b51d7
• When the temperature of a rigid hollow sphere containing 685 L of helium gas is held at 621 K, the pressure of the gas is #1.89*10^3# kPa. How many moles of helium does the sphere contain?
• What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?
• Question #1a4dd
• Using the ideal gas formula, calculate the volume of 1.50 moles of a gas at 115 kPA and a temperature of 298K?
• Find the number of #"CO"_2# that exert a pressure of #"785 torr"# at a volume of #"32.5 L"# and a temperature #32^@"C"#?
• What does #R# mean in an organic formula?
• What is the temperature of a 25.0 g sample of neon gas that exerts a pressure of .922 atm and has a volume of 3.25 L?
• What pressure is exerted by 0.450 mol of a gas at 25 degrees Celsius if the gas is in a 0.50 L container?
• What is the volume occupied by 20.7 g of argon gas at a pressure of 1.04 atm and a temperature of 409 K?
• Question #91cb4
• At what Kelvin temperature will a sample of gas occupy 12 liters if the same sample occupies 8 liters at 27 ℃?
• What is the molar mass of a gas that has a density of 1.18g/L at 25°C and 1 atm?
• What mass of zinc metal is required to evolve a #30*mL# volume of dihydrogen gas from a #30*mL# volume of hydrochloric acid at #1.00*mol*L^-1# concentration?
• A sample that contains 3.66 mol of a gas at 265 K has a pressure of 1.09 atm. What is the volume?
• A sample of nitrogen gas is collected over water at a temperature of 23.0°C. What is the pressure of nitrogen gas if atmospheric pressure is 785 mm Hg?
• Question #c6b11
• Question #66004
• Question #2cbc3
• Question #c8a2e
• Why is Kelvin used in the ideal gas law?
• Why is the ideal gas law used?
• Why does ideal gas law fail at times?
• What is the ideal gas law used for?
• What does the ideal gas law state?
• What does the ideal gas law mean?
• How do chemists use the ideal gas law?
• How can you derive the ideal gas law?
• Does the ideal gas law apply to liquids or solids?
• How can the ideal gas law can be simplified?
• How can the ideal gas law be made more precise?
• How many moles of a gas would occupy #157# #L# at #132# #kPa# and #-16.8°C#?
• Question #359b2
• Question #575a0
• When do real gases behave most like ideal gases?
• What is the pressure of 25 moles of #H_2# gas in a 2 liter container at 35°C?
• If 98.5 mol of an ideal gas is at 1.73 atm and 477 K, what is the volume of the gas?
• If an ideal gas has a pressure of 2.65 atm, a temperature of 92.55 °C, and has a volume of 51.43 L, how many moles of gas are in the sample?
• What is the pressure of 0.540 mol of an ideal gas at 35.5 L and 223 K?
• Question #7af06
• What volume will 2.0 moles of nitrogen occupy at 720 torr and 20°C?
• Question #e3d46
• A 0.310 mol sample of xenon gas has a volume of 22.0 L at a pressure of 0.470 atm. What is the temperature of the gas in degrees Celsius?
• An engineer pumps 200.50 grams of carbon monoxide (CO) gas into a cylinder capacity of 120.0 L. What is pressure inside the cylinder at 45.0°C?
• Question #9b58c
• Under what pressure is chloroform at a mercury reading of #940*"Torr"#?
• In the ideal gas equation, which term is always constant?
• What volume would 5 moles of Helium occupy at 278°C and 765 mmHg?
• The air in lungs has 0.153 mol of gas particles at 302 K and 101.3 kPa of pressure. What is the volume of the air?
• A 2.00 L container holds .700 mol of oxygen gas at 285 K. What is the pressure in atm inside the container?
• What is the volume, in liters, occupied by 0.723 mol of a gas at 32.0°C if the pressure is 852 mm Hg?
• How many oxygen molecules are in 22.4 liters of oxygen gas at 273 K and 101.3 kPa?
• What is the approximate temperature of a 0.50 mol sample of gas at 750 mm Hg and a volume of 12 L?
• Question #9628d
• A spherical balloon can hold 1.2 liters of helium. The balloon has a mass of 26 milligrams when empty. Helium has a density of 0.1785 grams per liter. What is the mass of the balloon when it is filled with helium?
• 3.45 g of an unknown gas at 55°C and 1.10 atm is stored in a 2.55-L flask. What is the density of the gas?
• A sample of nitrogen gas stored in 4.0L container at 32°C exerts a pressure of 5.0 atm. What is the number of moles of nitrogen gas in the container?
• What is the pressure exerted by 43 mol of nitrogen in a 65 L cylinder at 5°C?
• What is the volume of 0.140 g of #C_2H_2F_4# vapor at 1.06 atm and 14.2°C?
• Question #bc2c7
• How many moles of oxygen are present in 33.6 L of the gas at 1 atm and 0°C?
• A hot air balloon has a volume of 500.0 L. At what temperature is the gas if there are 25 moles present at standard pressure?
• If a sample of gas which weighs 0.400 g has a volume of 250 mL at STP, what is the molecular weight of the gas?
• Why is helium an ideal gas?
• Which flask contains gas of molar mass 30, and which contains gas of molar mass 60?
• A sample of gas weighing 0.0286 g occupies a volume of 50 #cm^3# at 76 cmHg. and 25 degree centigrade. What is the molar mass of the gas?
• If 2.31 g of the vapor of a volatile liquid is able to fill a 498 ml flask at 100 degrees C and 775 mmHg, how do you calculate the molar mass of the liquid? Also, how do you calculate the density of the vapor under these conditions?
• What is the molecular mass of a compound if 560mL have a mass of 1.10g at STP?
• How was the ideal gas equation, #PV = nRT#, derived?
• How do you calculate the temperature of the gas at this new pressure?
• If 9.69 moles of an ideal gas has a pressure of 3.10 atm, and a volume of 64.51 L, what is the temperature of the sample?
• If 2.35 moles of an ideal gas has a pressure of 3.63 atm, and a volume of 68.93 L, what is the temperature of the sample in degrees Celsius?
• If 49.5 moles of an ideal gas occupies 37.5 liters at 479 K, what is the pressure of the gas?
• If 91.5 mol of an ideal gas occupies 69.5 L at 31.00°C, what is the pressure of the gas?
• If an ideal gas has a pressure of 4.97 atm, a temperature of 481 K, and has a volume of 29.83 L, how many moles of gas are in the sample?
• What is the pressure in a 10.6-L cylinder filled with 11.2 g of oxygen gas at a temperature of 345 K?
• Question #e9190
• What is the volume of the container needed to store 0.8 moles of argon gas at 5.3 atm and 227°C?
• What is the temperature of a 100 liter container having 1 mole of an ideal gas at a pressure of 20 kilopascals?
• Exactly one mole of an ideal gas is contained in a 2.00 liter container at 1,000 K. What is the pressure exerted by this gas?
• A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15°C. How many gas particles are in this bubble?
• How many moles of #NH_3# are in a 3.0 L vessel at #3*10^2# #K# with a pressure of 1.50 atm?
• A steel tank with a volume of 9.583 L contains #N_2# gas under a pressure of 4.972 atm at 31.8°C. How many moles of #N_2# are in the tank?
• If four moles of a gas of 5.4 atmospheres have a volume of 120 liters, what is the temperature?
• A 250 mL sample of oxygen is collected over water at 25°C and 760.0 torr pressure. What is the pressure of the dry gas alone?
• Question #d9052
• Question #48160
• Question #4c1cf
• If 1.00 L of an unknown gas at STP has a mass of 5.40 g, what is its molar mass?
• What is the pressure inside a tank that has a volume of #1.20 * 10^3# L and contains 12.0 kg of #HCl# gas at a temperature of 18°C?
• What is the celsius temperature of 100.0 g of chlorine gas in a 40.0-L container at 800 mm Hg?
• Hydrogen is collected over water at 19C and 785 mmHg of pressure. THe total volume of the sample was 1.93L How do you calculate the volume of hydrogen at STP?
• Why do ideal gases exist?
• Is water an ideal gas?
• Is helium an ideal gas?
• Which of the following compounds will behave least like an ideal gas at low temperature? Why so?
• Under what conditions is a gas closest to properties of an ideal gas? Why?
• An ideal gas is made up of gas particles that have what properties?
• The boiling point of liquid nitrogen is -196 Celsius. On the basis of this information alone, is nitrogen an ideal gas?
• What is the proof of the ideal gas law?
• Hydrogen is collected over water at 0.975 atm and 28°C. What is the partial pressure of #H_2#?
• Question #aea36
• At what temperature will 14.0 g of #H_2# occupy a volume of 15.5L at a pressure of 204 kPa?
• If you have a gas at a pressure of 16.5 atm, volume of 123.9 mL, and a temperature of 11°C, how many moles do you have?
• Question #a9643
• If the volume of the container is #"1.00 L"#, what is the change in mols of gas required to change the pressure from #"1.00 atm"# to #"0.920 atm"# if the temperature was also dropped from #25^@ "C"# to #22^@ "C"#? (#R = "0.082057 L"cdot"atm/mol"cdot"K"#)
• Question #b85cd
• What is the volume of a container that holds 9.67 moles of oxygen gas at 100°C and 1.30 atm pressure?
• Which of these is true for ideal gases?
• If the pressure is #8.314 * 10^4# #Pa#, #R# is #8.314#, the temperature is #100# #K#, and the number of moles of gas (#n#) is #300#, what is the volume of a gas in #m^3#?
• What is the pressure (atm) of 3.5 moles of helium at -50 °C in a rigid container whose volume is 25.0 L?
• Question #e26c0
• Question #61c8a
• A neon gas in a sign has a volume of 42.5 L at 25 °C and 3.5 kPa. What is the mass of neon?
• Question #3f2c0
• A gas sample of #Xe# occupies 10-liter balloon at 27°C under a pressure of 1.2 atm. Approximately what volume would the gas occupy at 350 K at 2 atm of pressure?
• Oxygen gas is collected in a 5.00-liter container at 25°C and 380 torr. How many moles of oxygen are present in the container?
• A sample of 80 g of argon gas is at a temperature of 30°C and a pressure of 4 atm. What is the volume of the gas?
• What is the molar mass of a .250 gas that occupies 1.01 L at 31°C and 1.44 atm?
• How many grams of oxygen gas present in a 2.50-L sample kept at 1.66 atm pressure and a temperature of 10.0°C?
• What is the molar mass of a gas that has a density of 1.02 g/L at 0.990 atm pressure and 37°C?
• What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?
• How many moles of gas occupy a 3.45-L container at a pressure of 150 kPa and a temperature of 45.6°C?
• How many moles of gas are contained in 1.25 L at 303 K and 1.10 atm?
• How is this chemical Kinetics problem solved? (Deals with pressure along with the concentration)
• Question #64a0e
• What pressure, in atmospheres, is exerted by 0.325 moles of hydrogen gas in a 4.08 L container at 35°C?
• What volume is needed to store 0.80 moles of helium gas at 204.6 kPa and 300 K?
• Why do real gases deviate from the ideal gas laws at low temperatures?
• For real gases, how does a change in pressure affect the ratio of PV to nRT?
• For which gases does the ratio of PV to RT equal a constant?
• What pressure will be exerted by 2.01 mol hydrogen gas in a 6.5 L cylinder at 20°C?
• Question #92355
• A gas cylinder with a volume of 3.00 #dm^3# contains 8.00 moles of oxygen gas at a temperature of 50.0 K. What is the pressure inside the cylinder?
• How many moles of chlorine gas are contained in a 5.00 L flask at 27°C and .947 atm pressure?
• When an airbag is inflated the nitrogen gas has a pressure of 1.30 atmospheres, a temperature of 301 K, and a volume of 40.0 liters. What is the volume of the nitrogen at STP?
• Question #732f1
• Question #d4d89
• A balloon is inflated with 0.2494 g of helium to a pressure of 1.26 atm. If the desired volume of the balloon is 1.250 L, what must the temperature be in °C?
• A 5.00 L flask contains 0.02 moles oxygen at 22°C, what is its pressure, in kilopascals? What is the pressure in atm?
• Ten moles of a gas are contained in a 1.00 L container at 295 K. What is the pressure of the gas?
• What is the density of water vapor at room temperature?
• Question #5d930
• What volume would be occupied by a #0.1*mol# quantity of gas at a temperature of #310*K#, and a pressure of #700*mm*Hg#?
• What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?
• What is the total pressure in a 6.00-L flask which contains 0.127 mol of #H_2# (g) and 0.288 mol of #N_2# (g) at 20.0°C?
• How many mL of #O_2# gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of #KClO_3#?
• Question #f9d12
• What is the density of methane at 28.5°C and 755.2 mmHg?
• What is the pressure of 4 moles of helium in a 50 L tank at 308 K?
• How do you decide when to use this equation: pV=nRT?
• How do you use pV=nRT in chemistry?
• How does the ideal gas law relate to scuba diving?
• How does the Ideal gas law relate to hot air balloons?
• How does the Ideal gas law relate to real gases?
• If 64 grams of #O_2# gas occupy a volume of 56 liters at a temperature or 25°C, what is the pressure of the gas, in atmosphere?
• 0.345 moles of #CH_4# is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?
• What volume is occupied by 0.963 mol of #CO_2# at 300.9 K and 913 mmHg?
• If an Ideal gas has a pressure of 9.75 atm, a temperature of 323 K, and has a volume of 33.81 L, how many moles of gas are in the sample?
• What is the density of chlorine gas at 1.21 atm and 34.9°C?
• What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?
• What is the volume of #9.783*10^23# atoms of Kr at 9.25 atm and 512K?
• What is the volume of 2.10 moles of chlorine gas (#Cl_2#) at 273 K and 1.00 atm?
• A cylinder containers 27.5 L of oxygen gas at a pressure of 2.0 atm and a temperature of 320K. How much gas (in moles) is in the cylinder?
• Question #df0fe
• What is the pressure of a sample of #CH_4# gas (6.022 g) in a 30.0 L vessel at 402 K?
• A 425 mL volume of hydrogen chloride gas, #HCl#, is collected at 25°C and 720 torr. What volume will it occupy at STP?
• Question #44e55
• How many grams of helium are contained in a #"2.0-L"# balloon at #30.0^@"C"# and at #"735 mmHg"# ?
• How do you calculate the number of mol of a gas that is present in a 5.67 L container at 44.7 C, if the gas exerts a pressure of 614.0 mmHg.?
• A 12.0 L gas cylinder has been filled with 5.40 moles of gas. You measure the pressure to be 3.10 atm What is the temperature inside the tank?
• A 16.0 L gas cylinder is filled with 7.60 moles of gas. The tank is stored at #27^oC#. What is the pressure in the tank?
• Question #ccbc8
• In the ideal gas law equation, #PV=nRT#, what is the value of the variable #'R'#?
• After burning 1.5g of some gas, 4.4g of CO2 and 2.7g of H2O were produced. What is this gas if at STP 1L of this gas weighs 1.34g?
• What is the difference between an ideal gas and a real gas?
• Question #ca88b
• Question #52822
• When is deviation from the ideal gas law greatest?
• On a PV diagram, suppose we place volume on the #y# axis; is the slope negative or positive?
• What volume of dioxygen gas would result from decomposition of potassium chlorate at #27# #""^@C#?
• In an ideal gas mixture, how does each individual affect the other gases in the mixture?
• Question #bde13
• Question #262d6
• Question #0c37e
• (p+a/v^2)v=RT,derive the cyclic rule.i.e. show the products of the partial derivatives of p,v&T taken in a order is equal to -1?
• If the initial temperature of an ideal gas at 2.250 atm is 62.00 #"^o#C, what final temperature would cause the pressure to be reduced to 1.500 atm?
• If 37.5 mol of an ideal gas occupies 38.5 Lat 85.00°C, what is the pressure of the gas?
• Question #35c5e
• Question #d132b
• What pressure is exerted by a #10*g# mass of nitrogen gas?
• The reaction of magnesium with hydrochloric acid at 30 °C and 817.36 mmHg produced 4.03 L of hydrogen that was collected over water. The vapour pressure of water at 30 °C is 33.4 mmHg. How many moles of hydrogen were formed?
• Question #1414a
• How many molecules are in 22.41 L of an ideal gas at STP?
• How did the ideal Gas Law originate?
• Question #de7e1
• Question #f51ce
• Question #c3cd4
• Question #831b6
• A #780*mL# volume of gas #1.00*atm# pressure, and #310*K# temperature, is cooled to #295*K#, and #65*mm*Hg# pressure. What is the new volume?
• Question #aac0d
• An unknown gas at 49.1 °C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas?
• Molar mass and density?
• Question #d4ecd
• What is the volume occupied by a #91.8*g# mass of carbon dioxide that is heated to #517.2*K#, and subjected to a pressure of #287*"Torr"#?
• Question #0dfe4
• A sample of gas has a mass of 0.565 g. Its volume is 117 mL at a temperature of 95 C and a pressure of 749 mm Hg. How would you find the molar mass of the gas?
• A sample of neon has a volume of 75.8 at STP. How many moles are present?
• What mass of fluorine gas generates a pressure of #375*"Torr"# when confined to a #5.12*L# volume at #298.9*K#?
• Question #fc809
• Question #e9ae8
• How do you calculate #DeltaS_(sys)# for the isothermal expansion of 1.5 mol of an ideal gas from 20.0 L to 22.5L?
• Question #aea28
• How many air molecules are in a room whose dimensions are #13.5*ftxx12.0*ftxx10.0*ft# at a temperature of #20# #""^@C#?
• A volume of 50.0 milliliters of an ideal gas at STP increases to 100 milliliters. If the pressure remains constant, what must the new temperature be?
• Question #29d0f
• A 0.642 g sample of an unknown gas was collected over water at 25.0 degrees C and 1.04 atm. The collection cylinder contained 151.3 mL of gas after the sample was released. How do you find the molar mass of the unknown gas?
• How to claculate value of universal gas constant?
• What is the volume composition of this gas mixture?
• What pressure is exerted by a mass of #1*g# nitrogen gas that is contained in a #0.50*L# volume under standard conditions?
• Under what conditions of temperature and pressure does oxygen gas behave least like an ideal gas?
• Question #38d7c
• Question #74d82
• How much carbon monoxide will result if #222*kg# of carbon are combusted to give #5/8# equiv of carbon monoxide?
• What is the atomic mass of a gas that has #rho=2.50*g*L^-1# at a pressure of #0.974*atm#, and a temperature of #371*K#?
• What volume would a MASS of #3.60*g# hydrogen gas occupy under standard conditions?
• What volume will #1.50*mol# of an Ideal Gas occupy at #225*K#, at a pressure of #231*mm*Hg#?
• Ammonia gas occupies two containers. One volume is TWICE the volume of the other. Given that the containers are under the same pressure AND same temperature, how many molecules are in the second volume if the first volume contains #6xx10^23# particles?
• How do the gas laws operate in scuba diving? I mean to exclude the rule of never holding your breath...
• Question #9cb33
• Question #ffdb3
• Question #d190a
• How many moles of gas are contained in 890.0 mL at 21.0 °C and 750.0 mmHg pressure?
• Question #42191
• Question #dd0b7
• What is the meaning of ideal gas?
• What is the density of neon gas given a pressure of #505*mm*Hg#, and a temperature of #318*K#?
• A sample of diatomic gas A has three times the mass of an equal volume of gas B under the same conditions. What is the ratio of the atomic mass of A to that of B?
• Question #e4692
• Question #2828a
• Question #79862
• What is the volume expressed by a #74.3*g# mass of carbon dioxide at #294.9*K# enclosed in a piston at a pressure of #439*"mm Hg"#?
• Which gas at #150^@ "C"# is more ideal at #"1 atm"#, water or methane?
• A #0.20*g# mass of gas occupies a #0.200*L# volume at one atmosphere, and #300*K#. What is the molar mass of the gas?
• Question #99984
• What is the molar quantity of a gas at #742*mm*Hg# pressure, at #298.0*K# temperature, confined to a volume of #6.0*L#?
• Question #d33e2
• Question #5ea04
• A gas has a density of #3.18*g*L^-1# at a temperature of #347*K#, and a pressure of #1.2*atm#. What is its molecular mass?
• A #0.275*L# volume of an unspecified gas exerts a pressure of #732.6*mm*Hg# at a temperature of #-28.2# #""^@C#. What is the molar quantity of this gas?
• If an ideal gas has a pressure of 7.05 atm, a temperature of 379 K, and has a volume of 54.75 L, how many moles of gas are in the sample?
• What is the pressure in atmospheres, if the pressure is reported to be #854*mm*Hg#?
• Question #ecf9c
• Question #617a1
• What is the change in volume for the reaction of #"16 g CH"_4# and #"16 g O"_2# at #700^@ "C"# and #"1 bar"#? The reaction is #"CH"_4(g) + 1/2"O"_2(g) -> "CO"(g) + 2"H"_2(g)#.
• Question #24a0b
• Question #0c095
• Question #51c75
• Question #5174b
• Question #17639
• Question #16856
• Question #95cad
• How do I choose which gas law to use???
• What is the molar mass of a gas that at #823*K# exerts a pressure of #31.89*kPa# in a volume of #56.0*mL#?
• A #0.5090*g# mass of gas exerts a pressure of #746*mm*Hg#, and occupies a volume of #0.1294*L# at a temperature of #364*K#? What is its molecular mass?
• Question #eafcf
• An #0.846*g# mass of gas exerts a pressure of #752*"Torr"#, and expresses a volume of #354*mL#, at a temperature of #100# #""^@C#. What is the molar mass of the gas?
• Vapour density of agas if it's density is 0.178g/L at NTP is?
• A #0.795*g# mass of gas is confined to a #1*L# volume at a temperature of #89# #""^@C# under a pressure of #771*mm*Hg#. What is the molar mass of the gas?
• A #9.95*mol# quantity of ideal gas is placed in a container of #208*L# volume at #1.26*atm# pressure. What is the temperature of the gas?
• Question #caa3e
• How do we use the Ideal Gas Equation to specify a gaseous density?
• Question #b21cc
• What is the mass of a #22.41*L# volume of ethane that has a pressure of #780*mm*Hg#?
• Question #0c593
• What pressure IN #"kilopascals"# is exerted by the DRY gas if it is has been collected over water at #75# #""^@C#, and the total pressure is #3.41*atm#?
• what volume will be occupied by 3.0 moles of H2 at 25°C and 1.03 ATM?
• Determine the density of chlorine gas at 22.0°C at 1 ATM?
• If 1 mole of H2 gas was collected under 294.2K and 746.7 mmHg, what volume will it occupy?
• (8.8400x10^-1) mol of an ideal gas has a pressure of (1.50x10^2) kPa and temperature of (2.5700x10^2) K. What is the volume of the gas?
• A weather balloon has a volume of (7.20x10^1) L when at the surface where the pressure is (9.3000x10^1) kPa and a temperature is (2.6000x10^2) K. (see more below)?
• Question #38dd5
• What is the density of a dioxygen gas at #840*"mm Hg"# pressure at a temperature of #291*K#?
• How many moles of gas are present in a gas cylinder at #18*atm# at a temperature of #123# #""^@C#?
• Question #b1da4
• A gas is found to have a density of #"1.80 g/L"# at #"76 cm Hg"# and #27^@ "C"#. The gas is?
• A #283.3*g# mass of an elemental gas #X# exerts a pressure of #3.2*atm# at a temperature of #300*K#, while it is enclosed in a #30*L# volume. What is the identity of the element?
• Question #90f5f
• Question #ad885
• Question #be045
• #0.250*mol# quantities of dinitrogen and sulfur dioxide are enclosed in a #2.5*L# vessel at a temperature of #300*K#. What are the partial pressures of each gas, and what is the total pressure?
• A mixture of propane and butane are confined in a bottle with a small hole. What is the rate of effusion of butane with respect to butane?
• What mass in #"mg"# of #"O"_2# gas is found in #"469.9 mL"# of it contained at #"755 mm Hg"# and #60^@ "C"#?
• What volume of hydrogen gas is obtained when #"43.39 g"# of sulfuric acid reacts with solid aluminum metal?
• How many mols of nitrogen gas are contained in a #"8.349 L"# container held at #"200.6 torr"# and #64^@ "C"#?
• Question #145c8
• Question #fbcc4
• Find the density of #"NH"_3# at #"800 mm Hg"# and #"298 K"#?
• Question #4fe76
• Question #5f0d5
• Question #077bf
• Determine the volume occupied by 2.50 g of hydrogen gas at a pressure of 828 mm of mercury and a temperature of 35.0 C ?
• Question #27cfc
• What is the density of a mixture of methane, ethane, propane, and n-butane at #130^@ "C"# and #"1 atm"#? What is its specific gravity?
• A tank used for compressed gas contains #9750*mol# oxygen gas, in a volume of #9750*L#, at a temperature of #34.9# #""^@C#...?
• Question #2f29b
• Question #43d81
• A balloon with a volume of #2.00L# is filled with helium gas at a temperature of #27.0˚C# and a pressure of #1.20 atm#. How many grams of helium are in the balloon?
• Calculate the molar mass in #"g"/"mol"#of diacetyl (butanedione) given that in the gas phase #100# degrees Celsius and #747# torr, a #0.3060# g sample of diacetyl occupies a volume of #0.111L#?
• Question #742bc
• At constant temperature and volume, a #0.2*mol# quantity of helium gas exerts a pressure of #22.7*kPa#. HALF this molar quantity of oxygen gas is injected, what is #P_"Total"#?
• Question #25bda
• A 3.6 mole sample of methane gas is kept in a 1.50 liter container at a temperature of 100°C. What is the pressure of the gas?
• Question #a9717
• What is the mass of #"5.6 L"# of #"O"_2"# at #23^@"C"# and #"8.16 atm"#?
• Question #95220
• Question #36ab0
• Question #e0eda
• Suppose 0.440 kg of ethane are burned in air at a pressure of exactly 1 atm and a temperature of 13.0 °C. What is the volume of carbon dioxide gas that is produced?
• What is the size of an ideal gas particle?
• Question #f9fe7
• How do I prove that the cyclic rule of partial derivatives applies to #P#, #T#, and #V#?
• At an altitude for which ambient pressure is #0.700*atm#, and a temperature of #270.15*K#, a balloon contains #3.00*mol# of gas... What is the volume of the balloon....?
• Question #4b1ce
• Question #02e7c
• How do you find the number of moles for a gas from temperature and pressure?
• Question #941d1
• A #3.49*g# mass of a gas occupies a volume of #4.48*dm^3# under standard conditions, what is the molar mass of the gas?
• Question #de30c
• What is the pressure in #mm*Hg# if a #4.0*g# mass of oxygen gas at #303*K# was confined to a container whose volume of #3000*mL#?
• Question #db16f
• An #8*g# mass of methane, and a #2*g# mass of dihydrogen gas, were enclosed in a piston. What volume with the gases occupy under standard conditions?
• A sample of chlorine gas is confined in a 3.93-L container at 407 torr and 21.0 degrees Celsius. How many moles of gas are in the sample?
• If 1.93 * 10^-3 mol of argon occupies a 65.8-mL container at 20 degrees Celsius, what is the pressure (in torr)?
• What is the density of Freon-11 (CFCl3) at 166 degrees Celsius and 5.92 atm?
• How do you calculate the molar mass of a gas at 347 torr and 77 degrees Celsius if 206 ng occupies 0.206 #mu#L?
• After 0.600 L of Ar at 1.29 atm and 223 degrees Celsius is mixed with 0.200 L of O2 at 535 torr and 106 degrees Celsius in a 400.-mL flask at 23 degrees Celsius, what is the pressure in the flask?
• Question #5b97a
• What is the temperature of 0.59 mol of gas at a pressure of 1.5 atm and a volume of 12.9 L ?
• Question #bf70b
• After 0.600 L of Ar at 1.47 atm and 221 degrees Celsius is mixed with 0.200 L of O2 at 441 torr and 115 degrees Celsius in a 400.-mL flask at 24 degrees Celsius, what is the pressure in the flask?
• Question #a9607
• What volume is occupied by a #7*g# mass of dinitrogen gas at a temperature of #300*K#, and a pressure of #750*mm*Hg#?
• At #NTP#, for a DIATOMIC gas, how many atoms constitute a #5.6*L# volume?
• How many molecules are there in an #11.2*L# volume of gas at #"NTP"#?
• What is the volume of #2*mol# of an Ideal Gas at #0# #""^@C#, and #1*atm#?
• Question #62744
• What molar quantity of gas occupies a volume of #25*L# under a pressure of #742*kPa# at a temperature of #295*K#?
• Show that #b = 4V# for a hard sphere potential?
• Question #a7871
• What is the molecular mass of a gas if 3.7 g of the gas at 25 °C occupy the same volume as 0.184 g of hydrogen at 17 °C and the same pressure?
• Question #265c0
• Given density in #"g/L"#, how to calculate molar volume?
• What is the density of wet air with 75% relative humidity at 1atm and 300K? Given : vapour pressure of #H_2O# is 30 torr and average molar mass of air is 29g/mol?
• What volume of dioxygen gas would be generated by complete decomposition of a #10*g# mass of #KClO_3#, under a pressure of #750*mm*Hg#?
• A 75.0 mL steel reaction vessel is filled with oxygen gas (O2) until the pressure reads 145 atm at 22C. How many moles of oxygen are in the container?
• What volume is occupied by a #2*mol# quantity of oxygen, nitrogen, and fluorine gases, at #300*K# under a pressure of #1.3*atm#?
• Question #ca2ba
• What volume is occupied by a #5.0*g# mass of ammonia that is placed in a piston and allowed to expand against a pressure of #740*mm*Hg# at a temperature of #50# #""^@C#?
• What is the density of a #0.196*g# mass of gas, confined to a #100*mL# volume?
• How many liters of oxygen will be obtained from the decomposition of 1 g of H2O2. if the gas is collected at 28 degrees celsius and 0.867 atm?
• At #"340 K"# and #"1 atm"#, #"N"_2"O"_4# is #66%# dissociated into #"NO"_2#. What volume would #"10 g"# of #"N"_2"O"_4# occupy under these conditions?
• Question #3ccd4
• If the initial temperature of an ideal gas at 2.250 atm is 62.00 °C, what final temperature would cause the pressure to be reduced to 1.600 atm?
• At 22.5 ºC and 1.25 atm pressure, a sample of carbon dioxide gas occupies a volume of 2.65 L. How many moles of the gas are present?
• Question #e7283
• Question #e9c20
• Question #08265
• An unknown element #"X"# with oxygen forms a gas compound #"X"_2"O"# whose density at #-120^@"C"# and a pressure of #"320 mmHg"# is #"1.809 g/L"#. What is element #"X"#?
• Question #a9f52
• What is the mass of calcium carbonate used in part a.?
• At #627^@"C"# and #"1 atm"#, #"SO"_3# is partially dissociated into #"SO"_2"# and #"O"_2# . If the density of the equilibrium mixture is #"0.925 g/L"#, what is the degree of dissociation?
• Do ideal gases forms solutions even they don't have intermolecular forces? please explain.