A monatomic ideal gas expands isothermally from $\left\{p_1, V_1, T_1\right\}$ to $\left\{p_2, V_2, T_1\right\}$. Then it undergoes an isochoric process, which takes it from $\left\{p_2, V_2, T_1\right\}$ to $\left\{p_1, V_2, T_2\right\}$. Finally the gas undergoes an isobaric compression, which takes it back to $\left\{p_1, V_1, T_1\right\}$. b) Write an expression for total $Q$ in terms of $p_1, p_2, V_1$, and $V_2$.

Suppose an ideal gas has pressure $p$, volume $V$, and temperature $T$. If the volume is doubled at constant pressure, the gas does work $W_{p=\text { const }}$ If instead the volume is doubled at constant temperature, the gas does work $W_{T=\text { const. }}$. What is the relationship between these two amounts of work done by the gas? a) $W_{p=\text { const }}<W_{T=\text { const }}$ b) $W_{p=\text { const }}=W_{T=\text { const }}$ c) $W_{p=\text { const }}>W_{T=\text { const }}$ d) The relationship cannot be determined from the information given.

A tire on a car is inflated fo a gauge pressure of $32 \mathrm{Ib}^1 \mathrm{in}^2$ at a temperature of $27^{\circ} \mathrm{C}$. After the car is driven for $30 \mathrm{mi}$, the pressure has this polnt? a) $40.7 \mathrm{C}$ b) $23^{\circ} \mathrm{C}$ c) $32^{\circ} \mathrm{C}$ d) $54^{\circ} \mathrm{C}$

In a diesel engine, the fuel-air mixture is compressed rapidly. As a result, the temperature rises to the spontaneous combustion temperature for the fuel, causing the fuel to ignite. How is the rise in temperature possible, given the fact that the compression occurs so rapidly that there is not enough time for a significant amount of heat to flow into or out of the fuel-air mixture?

Explain why the average velocity of air molecules in a closed auditorium is zero but their root-mean-square speed or average speed is not zero.

When you blow hard on your hand, it feels cool, but when you breathe softly, it feels warm. Why?