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This chapter discusses the properties of gases and the mean free paths of molecules. It also explores the increase in molecular speed and its effect on average translational kinetic energy. Additionally, it covers the degrees of freedom of a bead on a wire and thermal interactions between systems. Finally, it examines entropy and the second law of thermodynamics.
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The table shows the properties of four gases, each having the same number of molecules. Rank in order, from largest to smallest, the mean free paths of molecules in these gases.
The table shows the properties of four gases, each having the same number of molecules. Rank in order, from largest to smallest, the mean free paths of molecules in these gases.
The speed of every molecule in a gas is suddenly increased by a factor of 4. As a result, vrms increases by a factor of 1. 16. 2. >4 but not necessarily 16. 3. 4. 4. <4, but not necessarily 2. 5. 2.
The speed of every molecule in a gas is suddenly increased by a factor of 4. As a result, vrms increases by a factor of 1. 16. 2. >4 but not necessarily 16. 3. 4. 4. <4, but not necessarily 2. 5. 2.
Which system has the largest average translational kinetic energy per molecule? 1. 1 mol of He at p = 1 atm, T = 300 K 2. 2 mol of N2 at p = 0.5 atm, T = 450 K 3. 2 mol of He at p = 2 atm, T = 300 K 4. 1 mol of Ar at p = 0.5 atm, T = 450 K 5. 1 mol of N2 at p = 0.5 atm, T = 600 K
Which system has the largest average translational kinetic energy per molecule? 1. 1 mol of He at p = 1 atm, T = 300 K 2. 2 mol of N2 at p = 0.5 atm, T = 450 K 3. 2 mol of He at p = 2 atm, T = 300 K 4. 1 mol of Ar at p = 0.5 atm, T = 450 K 5. 1 mol of N2 at p = 0.5 atm, T = 600 K
How many degrees of freedom does a bead on a wire have? 1. 1 2. 2 3. 3 4. 4 5. 5
How many degrees of freedom does a bead on a wire have? 1. 1 2. 2 3. 3 4. 4 5. 5
Systems A and B are interacting thermally. At this instant of time, 1. TA = TB. 2. TA > TB. 3. TA < TB.
Systems A and B are interacting thermally. At this instant of time, 1. TA = TB. 2. TA > TB. 3. TA < TB.
Two identical boxes each contain 1,000,000 molecules. In box A, 750,000 molecules happen to be in the left half the box while 250,000 are in the right half. In box B. 499,900 molecules happen to be in the left half the box while 500,100 are in the right half. At this instant of time, 1. The entropy of box A is smaller than the entropy of box B. 2. The entropy of box A is equal to the entropy of box B. 3. The entropy of box A is larger than the entropy of box B.
Two identical boxes each contain 1,000,000 molecules. In box A, 750,000 molecules happen to be in the left half the box while 250,000 are in the right half. In box B. 499,900 molecules happen to be in the left half the box while 500,100 are in the right half. At this instant of time, 1. The entropy of box A is smaller than the entropy of box B. 2. The entropy of box A is equal to the entropy of box B. 3. The entropy of box A is larger than the entropy of box B.
Chapter 18 Reading Quiz
What is the name of the quantity represented as vrms? 1. random-measured-step viscosity 2. root-mean-squared speed 3. relative-mean-system velocity 4. radial-maser-system volume
What is the name of the quantity represented as vrms? 1. random-measured-step viscosity 2. root-mean-squared speed 3. relative-mean-system velocity 4. radial-maser-system volume
What additional kind of energy makes CV larger for a diatomic than for a monatomic gas? 1. Charismatic energy 2. Translational energy 3. Heat energy 4. Rotational energy 5. Solar energy
What additional kind of energy makes CV larger for a diatomic than for a monatomic gas? 1. Charismatic energy 2. Translational energy 3. Heat energy 4. Rotational energy 5. Solar energy
The second law of thermodynamics says that 1. the entropy of an isolated system never decreases. 2. heat never flows spontaneously from cold to hot. 3. the total thermal energy of an isolated system is constant. 4. both 1 and 2. 5. both 1 and 3.
The second law of thermodynamics says that 1. the entropy of an isolated system never decreases. 2. heat never flows spontaneously from cold to hot. 3. the total thermal energy of an isolated system is constant. 4. both 1 and 2. 5. both 1 and 3.
In general, 1. both microscopic and macroscopic processes are reversible. 2. both microscopic and macroscopic processes are irreversible. 3. microscopic processes are reversible and macroscopic processes are irreversible. 4. microscopic processes are irreversible and macroscopic processes are reversible.
In general, 1. both microscopic and macroscopic processes are reversible. 2. both microscopic and macroscopic processes are irreversible. 3. microscopic processes are reversible and macroscopic processes are irreversible. 4. microscopic processes are irreversible and macroscopic processes are reversible.
