2. According to the kinetic theory, the substances that are made of particles are (a) ideal gases; (b) all gases; (c) all matter; (d) all matter except solids.
3. In an ideal gas, the Kelvin temperature (a) is directly proportional to the average kinetic energy (speed) of the gas; (b) is inversely proportional to the kinetic energy of the gas; (c) is a measure of the potential energy of the gas; (d) fluctuates widely when the gas is at equilibrium.
4. In an ideal gas the particles (a) occupy most of the space; (b) do not move; (c) undergo elastic collisions; (d) experience attractive forces .
5. An example of gas diffusion would be (a) filling a flat tire with air; (b) the odor of perfume spreading throughout air in a room; (c) a cylinder of oxygen stored under high pressure; (d) all of the above.
6. The ideal gas does not work well at low temperatures because the (a) volume is too small; (b) molecules are too far apart to have forces between them; (c) molecules are traveling too slowly to overcome forces between them; (d) pressure at low temperatures cannot be calculated.
7. The behavior of a gas under very high pressure is likely to (a) conform to the assumptions of the kinetic theory; (b) deviate from ideal gas behavior; (c) show, essentially, ideal gas behavior; (d) be nonpolar in nature.
8. If you know the temperature, volume, and quantity of a gas, you can calculate its (a) pressure; (b) formula; (c) condensation point; (d) flammability
9. To study the relationship between the temperature and volume of a gas, a factor that must be held constant is the gas's (a) elasticity; (b) fluidity; (c) kinetic energy; (d) pressure.
10. If the pressure of one mole of gas molecules remains constant while the temperature increases, then the volume occupied (a) increases; (b) decreases; (c) first decreases, then increases; (d) remains constant.
11. If the temperature of one mole of gas molecules remains constant and the volume available to the gas becomes larger, the pressure exerted by the gas (a) remains constant; (b) decreases; (c) increases; (d) increases then decreases.
12. If a constant force is applied but the surface is reduced, the pressure will (a) not change; (b) decrease; (c) increase;(d) increase or decrease, depending on the volume change.
13. The pressure exerted by a gas depends on the temperature, the volume, and (a) atmospheric pressure; (b) the number of particles of the gas present; (c) the type of gas involved; (d) the compressibility of the gas.
14. If the Celsius temperature is known, then the Kelvin temperature can be found using the equation (a) K = °C ‑ 273; (b) K = °C x 273; (c) K = 'C/273; (d) K = °C + 273.
15. If V, P, and T represent, respectively, the original volume, pressure, and temperature in the correct units, and V', P', and T' represent the new conditions, the gas‑law formula for this situation is (a) PV/T’ = P'V'/T' (b) PV'/T = P'V/T'; (c) P'V/T = PV'/T'; (d) PV/T = P'V'/T'
16. The lowest possible temperature, given a value of zero on the Kelvin scale, is referred to as
17. The average sea‑level pressure at 0 °C is defined as one of pressure.
18. A gas that does not obey completely all the assumptions of the ideal gas is called a(n)
19. The spontaneous mixing of two substances due to their random motion is referred to as
20. A(n) is a collision in which there is no net energy loss due to friction.
21. The idea that particles of matter are in constant motion is the basis for an important generalization in science called the
22. The pressure of a gas will if the temperature and number of moles of the gas remains constant but the volume decreases.