Equilibrium Constants

Key Questions

• Does equilibrium constant change with concentration?

  Answer:

  Equilibrium constant does not change with concentration.

  Explanation:

  The only variable that changes the equilibrium constant (also known as Kc) is Temperature.

  Me you · 1 · Jun 15 2018
• What are equilibrium constants?

  Equilibrium constants (Keq) are a way of the quotient of a reaction which has reached equilibrium.

  The equilibrium expression allows a calculation to be performed which tells us the levels of reactants vs. products.

  A large Keq means that the reaction REALLY favors the formation of products (forward reaction).

  A small Keq means that the reaction REALLY favors the formation of reactants (reverse reaction).

  Here are two videos to help with this concept:
  

  Video from: Noel Pauller

  Video from: Noel Pauller

  Noel P.

  mrpauller.weebly.com · 1 · Aug 26 2014

• How does the equilibrium constant change with temperature?
• How do you find equilibrium constant for a reversable reaction?
• Question #a90d2
• What is the equilibrium constant for the reaction of NH3 with water?
• What is the equation for finding the equilibrium constant for a chemical reaction?
• What is the equilibrium constant for the weak acid KHP?
• Consider this equilibrium: I2(s) + H2O(l) ⇌ H+(aq) + I-(aq) + HOI(aq). What is the Keq expression for this equilibrium?
• What is the equilibrium constant for water?
• What is the equilibrium constant of citric acid?
• What is the rate of production of reactants compared with the rate of production of products at equilibrium?
• What is the equilibrium constant of CH3COOH?
• How can I find the equilibrium constant of a reversed reaction?
• How can I find the equilibrium constant without concentrations?
• What are the units for the equilibrium constant?
• How does the value of an equilibrium constant relate to the relative quantities of reactants and products at equilibrium?
• If equilibrium constant is equal to 1, what does that mean?
• How is the equilibrium constant related to Gibbs free energy?
• Why are equilibrium constants dimensionless?
• Does equilibrium constant change with concentration?
• Does equilibrium constant affect the rate of reaction?
• What are equilibrium constants?
• Question #7bb00
• Question #34a11
• Question #c450e
• How is the value of the equilibrium constant useful?
• An amount of NO2 was initially put into a 5.0L flask. When equilibrium was attained according to the equation: 2NO (g) + O2 (g)--> 2NO2 (g), the concentration of NO was 0.800M. If Keq for this system is 24.0, what was the initial concentration of the NO2?
• Question #0ef5a
• Question #0ef97
• A 2.50ml aliquot of 0.0103 M Fe(NO3)3 is added to 2.50ml of 0.00101 M NaSCN and the following equilibrium is reached Fe(3+) + SCN(-) =FeNCS(2+). The concentration of FeNCS(2+) was determined to be 3.50 multiplied by 10(-4) M at equilibrium. Calculate Kc?
• Question #4fe75
• Question #fa88a
• Question #28d0a
• Question #05cf4
• Question #2c380
• Question #60f23
• What happens to the equilibrium constant in a complexation reaction?
• Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products #HCHO_(2(aq))+H_2O_((l))⇌H_3O_((aq))^(+)+CHO_(2(aq))^(-)#. Use A for #[HCHO_2]#, B for #[H_2O]#, C for #[H_3O^+]#, D for #[CHO_2^(−)]#?
• Question #586a5
• Question #e2b8b
• Question #b54e2
• For an equilibrium reaction, how can #K_c#, and #K_P# be related?
• Question #dcb75
• What happens to acetic acid at high temperature?
• Question #416e8
• Question #b23fd
• Question #22fd7
• Question #90a90
• Question #0f450
• Is #K_c# dependent on initial concentrations?
• At a certain temperature, 0.660 mol of SO3 is placed in a 4.50-L container, according to the reaction: 2SO3(g) --> 2SO2(g) + O2(g), at equilibrium, 0.130 mol of O2 is present, how would you calculate Kc?
• If enough of a monoprotic acid is dissolved in water to produce a 0.0150 M solution with a pH of 6.05, what is the equilibrium constant tor the acid?
• Question #050be
• For the dissociation of hydrogen cyanide in aqueous solution, i.e. #HC-=N(aq) + H_2O(l) rightleftharpoons H_3O^+ + ""^(-):C-=N#... which scenario will change the equilibrium constant?
• Question #92bdd
• The following reaction is at equilibrium at a particular temperature:#H_2(g) + I_2(g) -> 2HI(g)#. The #[H_2]_(eq) = .012 M, [I_2]_(eq) = .15 M#, and #[HI]_(eq) = .30 M#.What is the magnitude of #K_c# for the reaction?
• Lactic acid HC3H5O3 has one acidic hydrogen. A 0.10 M solution of lactic acid has the concentration of hydronium ion of 0.00363 M. Calculate Ka for lactic acid?
• In which reaction does kp=kc? a) NO(g)+O2(g) <-->N2O3(g) b) N2(g)+O2(g) <-->2NO(g) c) CaCO3(s) <-->CaO(s)+CO2(g) d) N2(g)+H2O(g) <-->NO(g)+H2(g) e) None
• In the reaction #N_2(g) + 3H_2(g) -> 2NH_3(g)#, #N_2 = 10.00 M#, #H_2 = 8.00 M#, and #NH_3 = 2.00 M#. What is the equilibrium constant #K#, for this reaction?
• Lactic acid has one acidic hydrogen. A 0.1 M solution of lactic acid has a pH of 2.44. Calculate Ka for lactic acid?
• A weak acid,HA has the concentration of C mol/dm and degree of dissociation ,β.Assuming Ka<<1, prove that β is inversely proportional to square root of C?
• A 0.10 M NH3 solution has a degree of dissociation 1.3% at temperature T. Calculate Kb for NH3 at this temperature?
• Write the expression for the equilibrium constant for the following reactions ? 2SO2(g) + O2(g) -------> 2SO3(g)
• What is #K_(eq)# for the reaction #N_2+3H_2 -> 2NH_3# if the equilibrium concentrations are #[NH_3] = 3.0 M, [N_2] = 2.0M#, and #[H_2] = 1.0M#?
• The pH of a 0.100 M solution of an aqueous weak acid (#HA#) is 4. What is the #Ka# for the weak acid?
• Question #b1be6
• Question #eece7
• Question #5f837
• How would you write the equilibrium constant expression for the following #H_2O_((g))# #rightleftharpoons# #H_2##(g)# #+# #1/2# #O_2##(g)# ?
• Question #6558e
• What is the equilibrium constant expression for the equation #C(s) + O_2(g) rightleftharpoons CO_2(g)#?
• Question #8cb12
• Question #dd381
• For the production of ammonia...#N_2(g)+3H_2(g) rightleftharpoons2NH_3(g)#..what is true at equilibrium...?
• Which one of the following equilibrium reactions corresponds to the β2 constant for the complexation reaction described above? Part a) Ag+(aq) + 2Cn^-1(aq)
• Question #44894
• The #pKa# of butyric acid #"HBut"# is 4.7. How do you calculate #K_b# for the butyrate ion #"But"^-#?
• Question #a8bc5
• Question #7b270
• Question #7cd04
• Question #f7401
• Find the equilibrium constant for a 3-electron transfer process, whose standard emf is #"0.59 V"# at #"298.15 K"#? #F = "96485.33 C/mol e"^(-)#
• What is the equilibrium constant of pure water at 25°C?
• Why is keq unitless?
• 6 moles of #"Cl"_2# are placed in a 3L flask at 1250K. At this temperature, #"Cl"_2# begins to dissociate into #"Cl"# atoms. What is the value for #K_c# if 50.0% of the #"Cl"_2# molecules dissociate when equilibrium has been achieved?
• How do you write the equilibrium expression for hydrolysis of a Lewis acidic metal cation?
• What happens when ammonia solution is heated? How does ammonia react as a base?
• Question #a750a
• How do you calculate Keq?
• How do you calculate Keq from pKa?
• How do you find the Keq equation?
• How do you write the Keq equation?
• What is the Keq equation?
• How do you calculate #K_"eq"# from #DeltaG^@#?
• How do you calculate Keq from equilibrium constants?
• How do you calculate Keq from pKa values?
• How do you calculate the Keq of a reaction?
• How do you calculate Ksp?
• What is Ksp?
• How do you solve Ksp in chemistry?
• How do you solve the Ksp equations?
• How do you set up a Ksp equation?
• How do you write the Ksp equation?
• What is the Ksp equation?
• How do you calculate Ksp from concentration?
• How do you calculate Ksp from solubility?
• How do you calculate Ksp if given molar solubility?
• How do you calculate Ka?
• How do you determine Ka?
• How do you write Ka?
• What is Ka in chemistry?
• What is the Ka chemistry constant?
• What is Kb and Ka in chemistry?
• What is Ka?
• Why is Ka important in chemistry?
• How do you calculate the Ka of an acid?
• How does Ka relate to acid strength?
• What happens to the equilibrium constant when a catalyst is added to the reaction mixture?
• What is the concentration of #"AlF"_6^"3-"# after mixing #"25 cm"^3# of 0.1 mol/L aluminium ion with #"25 cm"^3# of 1 mol/L fluoride ion?
• What is #K_a# for #HNO_2(aq) # ⇌ #H^+ (aq)# + # NO_(2^-)(aq)#?
• What does #K_(eq) # << 1 mean?
• Using the appropriate values of #K_(sp)# and #K _f#, what is the equilibrium constant for the following reaction: #PbCl_2(s) + 3OH^(-)(aq) rightleftharpoons Pb (OH)_3^(-)(aq) + 2Cl^(-)(aq)# ?
• What does a very large Keq indicate?
• How would you calculate K for the following equilibrium when [#SO_3#] = 0.0160 mol/L, [#SO_2#] = 0.00560 mol/L. and [#O_2#] = 0.00210 mol/L?
• In a reversible reaction. is it true that two substances are in equilibrium if the concentration of each increases by the same amount but the equilibrium constant remains unaffected?
• During the course of the reaction, the vessel is found to contain #"7.00 mols"# of #C#, #"14.0 mols"# of #H_2O#, #"3.60 mols"# of #CO#, and #"8.50 mols"# of #H_2#. What is the reaction quotient #Q#?
• Consider the following reaction: #Xe(g) + 2F_2(g) -> XeF_4(g)#. A reaction mixture initially contains 2.24 atm #Xe# and 4.27 atm #F_2#. lf the equilibrium pressure of #Xe# is 0.34 atm, how do you find the equilibrium constant (#K_p#) for the reaction?
• Question #88ec4
• Question #b2abc
• Question #c0a10
• Question #eedef
• How would you calculate the value of #K_p# for the equation #C(s) + CO_2(g) leftrightarrow 2CO(g)#?
• Write the equilibrium constant expression for the following reactions?
• Use the information below to answer the following question. What is the pH of a 0.100 M solution of benzoic acid?
• #CH_2H_3O_2(aq) + H_2O(l) rightleftharpoons H_3O^+ + C_2H_3O_2^-(aq)#. #K_c = 1.8 X 10^-5# at 25 #"^oC#. If a solution initially contains 0.210 M #HC_2H_3O_2#, what is the equilibrium concentration of #H_3O^+# at 25 #"^oC#?
• Consider the reaction: #NiO(s) + CO(g) rightleftharpoons Ni(s) + CO_2(g)#. #K_c = 4.0 xx 10^3# (at 1500 K). If a mixture of solid nickel (II) oxide and 0.10M carbon monoxide comes to equilibrium at 1500 K, what is the equilibrium concentration of #CO_2#?
• 9.2g of dinitrogen tetroxide is taken in a closed 1L vessel and heated till the following equilibrium is reached. At equilibrium, #50%# of the #"N"_2"O"_4(g)# is dissociated. What is the equilibrium constant (in mol/liter) ?
• A vessel at 1000K contains #"CO"_2# with a pressure of 0.5atm. Some of the #"CO"_2# is converted into #"CO"# on the addition of graphite. If the total pressure at equilibrium is 0.8atm, the value of #K_p# is?
• When I ask my calculator to divide #0.35# by #( 0.15 ) * ( 0.30 )^2# it gives me the result #0.21#. The correct result should be about #26#. What's going wrong?
• Using an ICE Table, how do we calculate #K_c# for the following reaction?
• What is the equilibrium constant for the following reaction at #"298 K"#? And what is the partial pressure of #"S"_8(g)# above #"S"(s, "orthorhombic")# at equilibrium at #25^@ "C"#?
• Question #1a1ea
• What is the equilibrium constant of #PCl_5 (g) -> PCl_3(g) + Cl_2(g)#?
• What is the equilibrium constant of #H_2O(g) + C(s) -> Co(g) + H_2(g)#?
• What is the equilibrium constant of #CH_3COOH(aq) + C_2H_5OH(aq) -> CH_3COOC_2H_5 (aq) + H_2O(l)#?
• I am really confused about the relationship between Kp and Kc?? (1) Kp = Kc (2) Kp > Kc (3) Kp<Kc Please explain me very easy methods with basics. thanks a lot.
• When 2 moles of hydrogen is heated with 2 moles of iodine,2.96 moles of hydrogen iodide is formed.what is the equilibrium constant for the formation of hydrogen iodide?
• For complex formation of iron(III) thiocyanate at a certain ionic strength, #K_f = 1099#. If its initial concentration is #"4.0 M"#, determine the equilibrium concentration of all species in solution for the dissociation of iron(III) thiocyanate in water?
• What is is #K_a# for #HCN(aq) rightleftharpoons H^+(aq) + CN^- (aq)#?
• Why is it necessary to maintain a constant temperature in an experiment to measure an equilibrium constant?
• Consider this reaction: #"N"_ 2(g) + "O"_ 2(g) rightleftharpoons 2"NO"(g)#. The equilibrium constant #K_P#, for the reaction is #1.0 xx 10^-15# at 25°C and #0.050# at 2200°C. Is the formation of nitric oxide endothermic or exothermic?
• Someone would be kind enough to help me with this exercise: #2"SO"_3(g) -> 2"SO"_2(g) + "O"_2(g)# ?
• In Ka (acid equilibrium constant) what do the concentrations on the other side represent?
• Given the equilibrium #A(g)rightleftharpoonsB(g)#, what occurs if ....?
• Question #e399c
• What is the equilibrium constant expression for the following reaction? #FeO(s) + H_2(g) rightleftharpoons Fe(s) + H_2O(g)#?
• If the reaction quotient, Q, for a reaction is less than the value of the equilibrium constant, K, for the reaction at a given temperature what must be converted to work for the system to reach equilibrium?
• Question #82dc7
• Question #e6c92
• Question #cc730
• What is #K_a# of #"ZnCl"_2# ?
• What is an expression for the acid ionization constant (#K_a#) for #H_2CO_3#?
• How do you write an expression for the acid ionization constant (#K_a#) for #HF#?
• How do you write an expression for the acid ionization constant (#K_a#) for #HCHO_2#?
• Question #0837e
• Question #0f696
• Question #353c0
• Question #0b1ae
• What is the Ka of an acid of 6M which has a pH of 2.5 at 277.5K ?
• Question #8349f
• Question #9ef8a
• Given that the solubility of #BaF_2# is #4.59xx10^(-2)*mol*L^(-1)# under standard conditions, what is #K_"sp"# for barium fluoride?
• Finding initial concentration by using Kc and equilibrium concentration?!
• Question #bd092
• Question #d1102
• Question #04928
• Question #909ba
• If the #"pH"# of an aqueous solution of ammonium chloride is #4.60#, what is the #K_h# value of #"NH"_4^(+)#?
• Question #904a3
• Question #0a42a
• Question #25ef1
• The Ka of a monoprotic weak acid is #2.08 xx 10^-3#. What is the percent ionization of a .194 M solution of this acid?
• What is #K_(eq)# for the reaction #N_2 + 3H_2 rightleftharpoons 2NH_3# if the equilibrium concentrations are #[NH_3] = 3 M#, #[N_2] = 2 M#, and #[H_2] = 1 M#?
• At what approximate temperature will an equimolar mixture of #N_2(g)# and #O_2(g)# be 3.0 % converted to #NO(g)#?
• Question #28ef9
• Question #ef994
• Question #3dd04
• Question #97654
• Question #4f54f
• 0.2 mole of A and 0.4 mile of B were reacted at a certain temperature and allowed to come to equilibrium . A+B---2AB The equilibrium mixture contained 0.1 mole of A, find Kc if volume of the container was 2 dm^3?
• Question #4e4c2
• Question #af614
• What is the equilibrium constant formula?
• What happens to the color of the #Fe^(2+)# when the equivalence point is reached?
• Use this equation to find the equilibrium constant?
• What is #K_2#...for #2CO(g) + O_2(g) rightleftharpoons 2CO_2(g)#?
• An equilibrium constant of 900 indicates?
• Question #10b17
• If given the information below, how do you calculate the #K_c# for the reaction #2HF(aq) + C_2O_4^(2-)(aq) rightleftharpoons 2F^(-)(aq) + H_2C_2O_4(aq)#?
• Question #9c730
• Question #644c6
• At #430^@"C"#, an equilibrium mixture consists of #0.020# moles of #"O"_2#, #0.040# moles of #"NO"#, and #0.96# moles of #"NO"_2#. Calculate #Kp# for the reaction, given the total pressure is #"0.20 atm"# ?
• Which option expresses the solubility equilibrium that operates for #Ni(OH)_2#? #1.# #K_"sp"=[Ni^(2+)][HO^-]# #2.# #K_"sp"=[Ni^(2+)][HO^-]^2# #3.# #K_"sp"=[Ni^(2+)]xx2[HO^-]# #4.# #K_"sp"=[Ni^(2+)]^2[HO^-]#
• Question #b158f
• In an equation element #"A"(s)rightleftharpoons 2"B"(g)+"C"(g)+3"D"(g)#. If the partial pressure of #"D"# at equilibrium is #P_1#, calculate the partial pressures of #"B"# and #"C"# . Also, calculate the value of #K_p# in terms of #P_1#?
• Question #562d1
• Question #5ecc9
• The #K_a# of carbonic acid is #4.3 xx 10^-7# #H_2CO_3 rightleftharpoons H^+ + HCO_3^-#. What does this mean for #H_2CO_3#?
• Question #58e5e
• Can someone help me with questions 1, 3, and 4? As soon as possible please, I have several questions regarding the properties of equilibrium constants.
• What is the ion-product constant, #K_w#?
• Question #5a42c
• When #"0.2 M"# of propionic acid dissolves in water, the #"pH"# was found to be #4.88#. Find the #K_a# of propionic acid?
• Question #74a96
• Question #23afe
• Question #9caae
• What is the Ka value of this citric acid + NaOH titration?
• How do I find #K# and #DeltaH# for the overall reaction? The overall reaction is: #"Ni"("CO")_4(g) + 4"H"_2"O"(g) rightleftharpoons "Ni"(s) + 4"CO"_2(g) + 4"H"_2(g)#
• Question #89bee
• Question #32cda
• What is the #K_b# for #HSO_4^(-)# if its #K_a# is #1.99#?
• How do you write the equilibrium expression for... #2N_2O(g)+O_2(g) rarr 4NO(g)#?
• Question #90689
• Question #c281d
• Question #d1319
• How do you solve #1.7xx10^(-1)=(x^2)/(0.60-x)# for #x#?
• What is the equilibrium constant for the reaction #2"CH"_ 2"Cl" _ (2(g)) rightleftharpoons "CH"_ (4(g)) + "CCl"_ (4(g))# ?
• Can someone help me please? I didn't do it right then I got it right. Thanks!
• Question #fd11c
• We know that #K_w=10^(-14)# at #298*K#. How would #K_w# evolve at #373*K#?
• How do you determine the equilibrium constant #K_c# for the reaction #X + 2Y rightleftharpoons Z#? The equilibrium concentrations are #"0.216 M"# for #Z#, #"0.06 M"# for #X#, and #"0.12 M"# for #Y#.
• Question #9a69f
• Question #36d09
• Question #fe19f
• Question #964ef
• Question #6abf7
• How to calculate #K_c#? #"N"_2(g) + "O"_2(g) rightleftharpoons 2"NO"(g) #
• Question #23e08
• The #"pH"# of a #"0.08 mol dm"^(-3)# solution of #"HClO"# is equal to #2.85#. Calculate the ionization constant of the acid?
• Under a particular set of conditions the reaction comes to equilibrium where the partial pressures of #N_2O_4# and #NO_2# are found to be #"0.6 atm"# and #"0.07"# atm respectively. Determine #K_p#?
• What is the #K_a# for a #"1.0-mol L"^(-1)# #"NH"_4^(+)# solution with a #"pH"# of #4.64# ?
• An equilibrium mixture of #"28 g"# #"H"_2# and #"140 g"# #"Br"_2# is heated in a #"4.01-L"# vessel at #"1400 K"#. At equilibrium, the vessel is found to contain #"1.1 g"# of #"HBr"#. Calculate #K_c# ?
• What is the equilibrium constant, #K_c#, for the reaction at this temperature?
• What is the value of Kc of the overall reaction after combining the two individual reactions?
• If #K_p = 2.4 * 10^(-3)# for the reaction below, then what is #K_c# ?
• The #K_c# for the equation shown below is #0.543# at #425^@"C"#. What is the value of #K_c# for the reverse equation?
• #40%# of #"PCl"_5# is not dissociated at #300^@"C"#. The reaction is carried out in a flask of #"1-L"# capacity. The value of #K_c# would be?
• When writing an equilibrium constant expression, do I include aqueous reactants and products or only gases?
• Equilibrium pressures question?
• #H_2# (g) + #F_2# (g) #\rightleftharpoons2HF# (g), find final values of #[H_2]_(eq)#, #[F_2]_(eq)#, and #[HF]_(eq)#?
• At a certain temperature, 4.0 mol #NH_3# is introduced into a 2.0 L container, and the #NH_3# partially dissociates to #2NH_3(g)\rightleftharpoonsN_2(g)+3H_2(g)#. At equilibrium, 2.0 mol #NH_3# remains. What is the value of #K_c#?
• Calculate the pH of a solution of 0.10 M #HF# that is also 0.15 M #HCN# if #K_a# for #HF# is #1.0xx10^-5# and #K_a# for #HCN# is #1.0xx10^-7#?
• For the reaction below, #K_p=81.9#. A reaction mixture contains #P_(I_2)=0.114# atm, #P_(Cl_2)=0.102# atm, and #P_(ICl)=0.355# atm. Find the equilibrium values for #P_(I_2)#, #P_(Cl_2)#, and #P_(ICl)#?
• Find #K_c# for the reaction below (see details)?