11. Balance the gaseous chemical equation: C3H8 + O2  CO2 + H2O
a. 1, 5, 3, 4
b. 2, 3, 4, 1
c. 2, 10, 6, 8
d. 4, 6, 8, 2
12. Which of the following is NOT a gas mixture?
a. Air
b. Smelly Farts
c. Chimney Fumes
d. Butane
13. In which of the following gas mixtures of N2 and He is the partial pressure of He the greatest?
a. 2 moles N2, 3 moles He
b. 3 moles N2, 1 moles He
c. 4 moles N2, 2 moles He
d. 5 moles N2, 5 moles He
14. Which of the following systems will have the greatest volume at STP?
a. 1.00 g N2 (MM = 28 g/mol)
b. 1.00 g NH3 (MM = 17 g/mol)
c. 1.00 g He (MM = 4 g/mol)
d. 1.00 g CO2 (MM = 44 g/mol)
15. Which of the following will contain the greatest number of molecules at 300K and 1 atm pressure?
a. 0.01 L
b. 0.10 L
c. 1.00 L
d. 10.0 L
16. How much carbon dioxide is there in a 3.4 L balloon at SATP?
a. 0.13 g
b. 6.1 g
c. 0.15 mol
d. 6.6 g
17. In the reaction 2H2 (g) + O2 (g)  H2O(l), how many liters of oxygen gas at STP will be needed to react with 10 L of hydrogen gas at STP?
a. 20.0
c. 5.00 L
b. 10.0 L
d. 100 L
18. Which of the following postulates of the Kinetic Molecular Theory for gases explains why gases exhibit pressure?
a. The molecules are in constant random motion
b. The distance between the molecules is great
c. The molecules collide with the walls of the vessel
d. The molecular kinetic energy depends on the temperature.
19. How will a velocity of a gas molecule vary if its molecular weight is increased from 32 g/mol to 64 g/mol?
a. It will increase.
c. It will double.
b. It will decrease.
d. Nothing happens.
20. Which of the following gases is the fastest: He, O2, CO2, NH3?
g. O2
c. He
h. CO2
d. NH3​