Question #9b58c
1 Answer
Explanation:
All you have to do here is use the molar mass of argon to determine how many moles you get in that
So, you know that argon has a molar mass of
Use this value to find the number of moles of argon present in your sample
#325color(red)(cancel(color(black)("g"))) * "1 mole Ar"/(39.9color(red)(cancel(color(black)("g")))) = "8.145 moles Ar"#
The ideal gas law equation looks like this
#color(blue)(|bar(ul(color(white)(a/a)PV = nRTcolor(white)(a/a)|)))" "# , where
At this point, the most important thing to do is make sure that you know the units used in the expression of the universal gas constant.
In your case, you can use the value
#R = 8.31color(white)(a)("Pa" * "m"^3)/("mol" * "K")#
http://www.cpp.edu/~lllee/gasconstant.pdf
This will allow you to plug the values given to you in the ideal gas law equation without doing any unit conversions.
As you can see, the pressure of the gas will be expressed in pascals,
#PV = nRT implies P = (nRT)/V#
Plug in your values to get
#P = (8.145color(red)(cancel(color(black)("moles"))) * 8.31("Pa" * color(red)(cancel(color(black)("m"^3))))/(color(red)(cancel(color(black)("mol"))) * color(red)(cancel(color(black)("K")))) * 298color(red)(cancel(color(black)("K"))))/(0.005color(red)(cancel(color(black)("m"^3))))#
#P = "4,034,023 Pa"#
Since you only have one sig fig for the volume of the gas, you can only have one sig fig for the resulting pressure
#P = color(green)(|bar(ul(color(white)(a/a)4 * 10^6"Pa"color(white)(a/a)|)))#