Question :
21. If the initial pressure of a 3.00 L gas : 1335480
21. If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?
A) 5.50 atm B) 2.50 atm C) 7.50 atm D) 1.88 atm E) 0.533 atm
22. Which of the following statements is incorrect? (Assume that pressure and amount of gas are constant.)
A)Charles’s law says that volume is directly proportional to temperature.
B)If the absolute temperature of a gas doubles, then the volume of the gas will double.
C)If the volume of a gas is halved, then the absolute temperature of the gas will be halved also.
D)If the temperature of a gas sample decreases from 50oC to 25oC, the pressure will be halved.
E)When a gas is cooled, the particles move more slowly.
23. If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will
A)become higher because of fewer collisions with the container.
B)become lower because of fewer collisions with the container.
C)become lower because of more collisions with the container.
D)become higher because of more collisions with the container.
E)stay the same because temperature has no effect on pressure.
24. If the temperature of a gas at a constant pressure is increased, the volume will
A)become smaller because of fewer collisions with the sides of the container.
B)become larger because of fewer collisions with the sides of the container.
C)become smaller because of more collisions with the sides of the container.
D)become larger because of more collisions with the sides of the container.
E)stay the same because temperature has no effect on pressure.
25. Charles’s Law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature. Which of the following is a consequence of Charles’s Law?
A)Oxygen cylinders are often used by climbers on Mt. Everest.
B)Underwater divers often use air cylinders.
C)Gases can be condensed to liquids at certain temperatures and pressures.
D)A sealed balloon will rise if the air in it is heated.
E)Application of sufficient pressure to carbon dioxide gas produces solid dry ice.
26. The pressurevolume relationship expressed by Boyle’s law can be explained by the kinetic molecular theory as follows:
A)When a gas is subjected to more pressure, more of the gas dissolves in a liquid.
B)When the volume of a gas is decreased, its molecules become closer together, causing more frequent collisions with the walls of the container.
C)The volume of a gas decreases as the pressure applied to the gas increases.
D)When the volume is decreased, the increased temperature causes the molecules to move faster and to hit the walls of the container more frequently.
E)The pressure of a gas results from its molecules being so close to one another that they cause the container walls to bulge.
27. Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0oC to 30.0oC.
A) 1.00 L B) 4.00 L C) 2.20 L D) 0.455 L E) 1.82 L
28. Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0oC to 30.0oC.
A) 1.17 L B) 10.5 L C) 4.19 L D) 2.92 L E) 1.75 L
29. A gas in a closed container with constant volume is heated from room temperature to 100°C. According to the kinetic molecular theory, the
A)average velocity of the molecules will increase.
B)gas will increase in weight.
C)individual molecules of the gas will increase their size.
D)average distance between molecules will increase.
E)pressure on the sides of the container will decrease.
30. Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0oC were to have a final volume of 1.50 L.
A) 2.0oC B) 127oC C) -146oC D) 9.8oC E) 43.2oC
