Chem 142, Autumn 2011
Name___________________
Section__________________
Group Activity 5: KMT, Real Gases, and Equilibrium
R = 0.08206 L·atm/mol·K
√
R = 8.314 J/mol·K
√
[
1 J = 1 kg·m2/s2
( ) ](
)
MM from the Periodic Table:
H (1.008 g/mol), He (4.003 g/mol), C (12.01 g/mol), O (16.00 g/mol), Ne (20.18 g/mol)
1. Kinetic Molecular Theory
a) At what temperature will urms for Ne(g) be the same as urms for He(g) at 300. K?
b) An unknown gas effuses from a container at a rate of 90.0 mL/min. An equal
volume of H2 in the same apparatus at the same temperature and pressure
effuses in at a rate of 400. mL/min. What is the molar mass of the unknown gas?
2. Real Gases
a) Use the van der Waals equation to calculate the pressure exerted by 1.00 mol of CO 2(g)
confined to a volume of 2.00 L at 273 K. a = 3.59 L2atm/mol2; b = 0.0427 L/mol
b) Use the van der Waals equation to calculate the pressure exerted by 1.00 mol of CO(g)
confined to a volume of 2.00 L at 273K. a = 1.49 L2atm/mol2; b = 0.0399 L/mol
c) Which gas (CO2 or CO) shows the greater departure from ideal gas behavior?
3. Balance the following reaction and write the equilibrium expression. Kc = 4.90 x 10-7 @ 60°C
H2S(g) +
I2(s)
HI(g) +
S(s)
If 0.050 moles of each reactant (H2S and I2) and 0.050 moles of each product (HI and S) are
added to a 2.00 L container, will the mixture be at equilibrium? If not, in which direction
will the reaction proceed to reach equilibrium?