The Gas Laws Worksheet

1.  For each of the following relationship, indicate the change:

As pressure increases, the temperature increases

As pressure increases, the volume decreases

As pressure increases, the number of moles increases

As temperature increases, the number of moles decreases

As pressure increases, the gas constant R stays the same

2.  For the following three relationships, indicate the law that describes the relationship:

V is inversely proportional to P _____Boyle’s______

V is directly proportional to T ______Charles’______

P is directly proportional to T __Gay-Lussac’s______

3.  At the buzzer, the Falcon basketball player throws the basketball into a cross-court arcing loop to the net. The ball slams into the background and fall through the net for 3 points. At the normal basketball pressure of 1.20 atm it has volume of 5.10 liters. At the impact with the backboard, the ball lost 2.50 liters of volume. What was the pressure of the basketball at this point? 2.35 atm

Problem #4-7 follow a story and may require information from previous problems.

4.  After making the new prototype pneumatic beachball of a novel game he created, Volley Vic, absent-mindedly, forgot how many moles of air he filled the ball with. If the ball he created could hold a volume of 100.0 liters at a pressure 2.50 atm when the temperature is 30.0˚ C at the beach, how many mole of gas are in the beachball?

10.0 mol

5.  Volley Vic took his new beachball to the beach where his friends laughed at him because this beachball was so large. He immediately left and cut several panels so the new volume was equal to 40.0 liters. After a quick calculation, what did he find the new number of moles of air to fill the ball to the same pressure to be? Assume that the other variables are kept the same. 4.02 mol

6.  After the change in design, this new ballgame of Volley Vic’s became a rage. It was found by Volley’s pals that if you hit the ball really hard, it sails for very long distances. Volley went to Paul Pressure to do some gas calculations to be sure his ball wouldn’t bust. They found that if you halved the new volume, the ball would indeed burst like a balloon. Paul was especially impressed with the pressure required to do this. Volley couldn’t see how Paul made the calculation. Show how much the pressure changes when the volume is halved assuming the other variables remain the same and report this pressure value. 5.00 atm

7.  The final model was snug under Volley’s arm as he arrived at the beach with Paul last weekend and ran into Bully Bart. Bar gave Volley’s ball mighty kick. With a quick estimation of the new volume of the ball at impact, Paul figured the ball’s volume was indeed halved by Bart. 1) If the temperature on this day was not 30.0˚C, but a cool 20.0˚C, did Bart bus Volley’s ball? (Assuming the other variables remain constant). 2) What was the new pressure upon impact? 3) Does the ball burst?

4.84 atm, No

8.  What is the value of the gas constant, R, when pressure is measured in mmHg and volume is measured in milliliters?

62,346 mmHg mL/mol K

9.  What volume will 25.0 g of oxygen gas occupy at 20.0˚C, and a pressure of 89.14 kPa?

21.3 L

10.  A 2.00 liter sample of a gas originally at 25.0˚C, and a pressure of 1.00 atm, is allowed to expand to a volume of 5.00 liters. If the final pressure of the gas is 0.770 kPa, what is its final temperature? 5.66 K

11.  A gas exerts a pressure of 0.329 atm at 20.0˚C. What pressure will it exert if its temperature is raised to 40.0˚C without change in volume?

0.351 atm

12.  A highly secretive flask of gasses contains 16.0 g of methane (CH4) and 16.0 g of Helium. The total pressure of the two gases is 0.567 atm and the temperature is 27.0oC. You may assume that the two gases do not react with each other.

a.  What is the number of moles of Helium in the flask?

b.  What is the partial pressure of Helium in the flask?

c. If the methane could be removed from the flask and the other conditions remained the same, what would be the total pressure exerted by the helium?

13. A mixture of N2 and O2 in a 0.200 liter container exerts a pressure of 0.948 atm at 35.0oC. If

there are 0.0020 moles of N2 present:

a. What is the partial pressure of N2?

b. What is the partial pressure of O2?

c. How many moles of O2 are present?

14. One Chunk: Real gases don’t always act like the ideal gases that are described so well by the ideal Gas Law. Why? Under what conditions don’t real gases behave like ideal gases?