1) 
If 300 mL of nitrogen at 280 mmHg were suddenly compressed into a 140 mL volume, what would be the final pressure?
Volume decreases so pressure increases. 

2) 
The temperature of 546 K is equivalent to:


3) 
The volume of a given sample of gas is 150.0 mL at 150°C and 1.0 atm pressure. Calculate the volume of the same gas sample at 10°C and 760 torr.
Temperature decreases so volume also decreases. 

4) 
A sample of Ar has a volume of 3.0 liters at 27°C. At what temperature would this sample have a volume of 5.0 liters? (P constant)
Volume increases so temperature increases. 

5) 
If the pressure in a steel gas cylinder is 37.5 atm at 22.0°C, what would the pressure be at a temperature of 300.0°C, as might be created in a fire?
Temperature increases so pressure increases. 

6) 
If the gas cylinder in question 5 were to burst at a temperature of 140.0 atm or greater, above what temperature would the integrity of the gas cylinder be in question?
This equation will find out the temperature when the pressure is 140 atm. Any temperatures greater than this will cause the container to burst. 

7) 
If 16.0g of He occupy 23.6 liters at some T and P, how many liters would 40.0 g of He occupy at the same T and P?
Because this is Helium at the same temperature and pressure, the grams and liters can be set up as a direct proportion. Alternately, you could solve for moles and use Avogadro's Law; moles increases so volume increases. 

8) 
Which one of the following statements is TRUE?
Choice A is not correct because standard temperature is 0°C. Choice C is not correct because the volume is 22.4 L. Choice D is not correct because standard temperature is 273 K. 

9) 
The density of a gas at STP was measured as 1.43 g/L. Which one of the following is a possible formula for the gas?
Since the gas is at STP, 22.4 L will be the volume of a mole. 32 g is the gmolar mass of O_{2}. 

10) 
If 1.12 L of an unknown gas has a mass of 3.55 g at STP, the gMM of the gas is:
Because this gas is at STP, 22.4 L is the volume of a mole. 

11) 
The volume of a gas weighing 0.55 g was found to be 210.0 mL when measured at 25°C and 740 torr. What is the gMM of this gas?
Alternately, you could solve for n using PV=nRT then plug the moles into MW=mass/mol 

12) 
The density of N_{2} at STP is:
Since this gas is at STP, the volume of one mole is at 22.4 L. 

13) 
The density of SO_{2} at 20.0°C and 740 torr is:
You cannot use 22.4 for the volume because the gas is not at STP. 

14) 
Calculate the volume of 2.00 moles of an ideal gas at a pressure of 0.100 atm and a temperature of 300.0 K.


15) 
How many molecules are in 2.0 L of hydrogen gas at 17°C and 780 torr?


16) 
Given: 4 NH_{3} + 5 O_{2} → 4 NO + 6 H_{2}
How many liters of NO are produced by the reaction of 10.0 liters of NH_{3} with 11.0 liters of O_{2}? ( All gases at the same T and P)
Since the gases are at the same temperature and pressure, their volumes will cancel. You can skip the liters to moles and the moles to liters steps. 

17) 
What volume of H_{2}, measured at STP, can be prepared by the electrolysis (decomposition) of 54.0 g of water?


18) 
Ten (10.0) grams of Na are placed into a flask containing 1.0 liter of Cl_{2} measured at STP. What is the maximum amount of NaCl that can form?
Since the gas is at STP the volume of one mole is 22.4 L. 

19) 
In a gaseous mixture of 1.0 mole of N_{2} and 4.0 moles of O_{2}, the total pressure is 0.20 atm. The partial pressure of N_{2} is.
Moles are directly proportional to the pressure. 

20) 
The rate of diffusion (effusion) of SO_{2} relative to the rate of diffusion of O_{2} at the same T and P is:
SO_{2} diffuses 0.71 times as fast as O_{2}. 

21) 
If a gas diffuses twice as fast as SO_{2} under the same conditions, its gMM is:


22) 
Which one of the following statements regarding the kinetic molecular theory of gases is incorrect?
When at the same temperature gases have the same kinetic energy, but they do not have the same velocity which is based on their molecular weight. 

23) 
Gases behave ideally at


24) 
Given: N_{2} + 3 H_{2} → 2 NH_{3}
How many liters of NH_{3} will be produced under 2.0 atm and 30°C, when 56.0 g of nitrogen react with excess hydrogen?
Since the gas is not at STP we cannot use 22.4 L for the volume of a mole. The volume must be calculated using PV=nRT. 

25) 
Given: N_{2} + 3 H_{2} → 2 NH_{3}
How many grams of nitrogen are required to produce 5.0 liters of NH_{3} under the conditions of 3.0 atm and 100°C?
Since the gas is not at STP we cannot use 22.4 L for the volume of a mole. The volume must be calculated using PV=nRT. 

26) 
Given 4 g He in a 10 L container and 44 g CO_{2} in a 10 L container
Which statement is correct if both containers are at STP?
Choice A is not correct because in the same volume CO_{2} weighs 11 times more than He. Choice B is not correct because Helium has a lower molecular weight and therefore has a higher velocity. Choice D is not correct because there are the same number of molecules in each container because they are at the same temperature, pressure and volume. 

27) 
Given: 2 moles of Ne and 3 moles of He in a 8 L container at 10.0 atm.
Which statement is correct?
Choice B is not correct because the gases have a pressure based on the number of moles in the container. Choice C is not correct because Ne has a pressure of 4 atm. Choice D is not correct because He has a pressure of 6 atm.

