What is Boyle's law?
a. Gas temperature is a constant.
b. Gas pressure is a constant.
c. The product of gas volume and gas pressure is a constant.
d. The product of gas temperature and gas pressure is a constant.
e. The sum of gas temperature and gas pressure is a constant.
[Ques. 2] Which of these is the ideal gas law that relates the temperature T, pressure P, and volume V of n moles of ideal gas consisting of N molecules?
a. PV = nRT
b. P = nRTV
c. PVn = RT
d. P = VRT
e. PV = NRT
[Ques. 3] Which of these is true about the absolute temperature of an ideal gas?
a. It is directly proportional to the average speed of the gas particles.
b. It is directly proportional to the average kinetic energy of the gas particles.
c. It does not depend on the average kinetic energy of the gas particles.
d. It is directly proportional to the volume of the gas particles.
e. It is directly proportional to the pressure of the gas particles.
[Ques. 4] This curve shows the distribution of atomic speeds calculated from an experiment in which particles of gas are projected through an apparatus as shown on page 217 of your textbook. How would the distribution of speeds change if the temperature of the gas were increased?
a. The shape of the distribution would remain qualitatively the same, but would shift to the right.
b. Same as answer a., except that the shift is to the left.
c. The distribution is not affected by temperature.
d. The peak gets higher without shifting over while the height of other parts of the curve decreases.
e. The peak gets lower without shifting over while the height of other parts of the curve increases.
[Ques. 5] Decreasing the volume of the container holding an ideal gas:
a. decreases the gas pressure by slowing the gas particles.
b. does not affect the gas pressure.
c. increases the gas pressure by slowing the gas particles.
d. increases the gas pressure because gas particles bounce off the walls of the container more often.
e. increases the gas pressure because gas particles strike the walls of the container with more momentum on average.
[Ques. 6] This figure depicts pollen grains suspended in a liquid exhibiting a continual, erratic motion known as Brownian motion. Albert Einstein inferred that atoms exist based on his calculations that described this type of motion. What was the basis for his conclusion?
a. The erratic motions of the pollen grains were explained by Einstein to result from random collisions with water molecules.
b. The tiny grains could be shown to be atoms.
c. The existence of atoms was an inescapable conclusion of his theory of relativity.
d. The existence of atoms was an inescapable conclusion of his theory of the photoelectric effect.
e. The existence of atoms was an inescapable conclusion of his theory of heat capacities of solids.
[Ques. 7] Which is NOT a characteristic of an ideal gas?
a. Its properties and behavior are identical to those of air at atmospheric pressure.
b. Its particles have no internal structure.
c. Its particles are indestructible.
d. Its particles only interact with each other when they collide.
e. It consists of an enormous number of tiny particles separated by large distances.
[Ques. 8] In chemistry and physics, what is a mole?
a. The number of grams of an element that equals its mass in atomic mass units.
b. The number of ounces of an element that equals its mass in atomic mass units.
c. The number of molecules of an element in a liter.
d. The number of atomic mass units of an element in a liter of its gas.
e. The number of atoms of an element in a liter.
[Ques. 9] What is one atomic mass unit?
a. The mass of a hydrogen atom at the Earth's surface.
b. The mass of an oxygen atom in outer space.
c. The mass of a carbon atom.
d. One-twelfth of a carbon atom.
e. One-twentieth the mass of a uranium atom.
[Ques. 10] What was Avogadro's hypothesis?
a. That under all conditions each liter of any gas contains the same number of molecules.
b. That under identical conditions each liter of all gases contains the same number of molecules.
c. That under ideal conditions each liter of all gases contains the same number of atoms.
d. That under identical conditions each liter of a particular gas contains the same number of molecules.
e. That under identical conditions each liter of all gases contains the same number of atoms.
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