A monatomic ideal gas expands slowly to twice its original volume, doing 450 J of work in the process. Find the heat added to the gas and the change in internal energy of the gas if the process is (a) isothermal; (b) adiabatic; (c) isobaric.

An air pump has a cylinder 0.250 m long with a movable piston. The pump is used to compress air from the atmosphere (at absolute pressure $1.01 \times 10^{5} \mathrm{Pa}$) into a very large tank at $3.80 \times 10^{5} \mathrm{Pa}$ gauge pressure. (For air, $C_{V}=20.8 J / \mathrm{mol} \cdot \mathrm{K}$.) (a) The piston begins the compression stroke at the open end of the cylinder. How far down the length of the cylinder has the piston moved when air first begins to flow from the cylinder into the tank? Assume that the compression is adiabatic. (b) If the air is taken into the pump at $27.0^{\circ} C$, what is the temperature of the compressed air? (c) How much work does the pump do in putting 20.0 mol of air into the tank?

A cylinder contains 0.0100 mol of helium at $T=27.0^{\circ} \mathrm{C}$. (a) How much heat is needed to raise the temperature to $67.0^{\circ} \mathrm{C}$ while keeping the volume constant? Draw a pV-diagram for this process. (b) If instead the pressure of the helium is kept constant, how much heat is needed to raise the temperature from $27.0^{\circ} \mathrm{C}$ to $67.0^{\circ} C$? Draw a pV-diagram for this process. (c) What accounts for the difference between your answers to parts (a) and (b)? In which case is more heat required? What becomes of the additional heat? (d) If the gas is ideal, what is the change in its internal energy in part (a)? In part (b)? How do the two answers compare? Why?

Nitrogen gas in an expandable container is cooled from $50.0\degree \mathrm{C}$ to $10.0\degree \mathrm{C}$ with the pressure held constant at $3.00 \times 10^5 \mathrm{~Pa}$. The total heat liberated by the gas is $2.50 \times 10^4 \mathrm{~J}$. Assume that the gas may be treated as ideal. Find
(b) the change in internal energy of the gas;

During an adiabatic expansion the temperature of 0.450 mol of argon (Ar) drops from $66.0^{\circ} C$ to $10.0^{\circ} \mathrm{C}$. The argon may be treated as an ideal gas. (a) Draw a pV-diagram for this process. (b) How much work does the gas do? (c) What is the change in internal energy of the gas?

A cylinder contains $0.0100$ mol of helium at $T=27.0\degree \mathrm{C}$.
($c$) What accounts for the difference between your answers to parts (a) and (b)? In which case is more heat required? What becomes of the additional heat?

A cylinder contains 0.100 mol of an ideal monatomic gas. Initially the gas is at $1.00 \times 10^{5} \mathrm{Pa}$ and occupies a volume of $2.50 \times 10^{-3} \mathrm{m}^{3}$. (a) Find the initial temperature of the gas in kelvins. (b) If the gas is allowed to expand to twice the initial volume, find the final temperature (in kelvins) and pressure of the gas if the expansion is (i) isothermal; (ii) isobaric; (iii) adiabatic.

A cylinder contains $0.0100$ mol of helium at $T=27.0\degree \mathrm{C}$.
(b) If instead the pressure of the helium is kept constant, how much heat is needed to raise the temperature from $27.0\degree \mathrm{C}$ to $67.0\degree \mathrm{C}$? Draw a $p V$-diagram for this process.

Six moles of an ideal gas are in a cylinder fitted at one end with a movable piston. The initial temperature of the gas is $27.0^{\circ} \mathrm{C}$ and the pressure is constant. As part of a machine design project, calculate the final temperature of the gas after it has done $2.40 \times 10^{3} J$ of work.

How can a complete sentence be made with the following statements?
Modelo: Yo creo que pueden venir. (es bueno): Es bueno que puedan venir.

Siguen las instrucciones del guía. (es importante)

A cylinder contains $0.0100$ mol of helium at $T=27.0\degree \mathrm{C}$.
(d) If the gas is ideal, what is the change in its internal energy in part (a)? In part (b)? How do the two answers compare? Why?

You blow up a spherical balloon to a diameter of 50.0 cm until the absolute pressure inside is 1.25 atm and the temperature is $22.0^{\circ} \mathrm{C}$. Assume that all the gas is $\mathrm{N}_{2}$, of molar mass 28.0 g/mol.

Find the mass of a single $\mathrm{N}_{2}$ molecule.

Two moles of an ideal gas are heated at constant pressure from $T=27^{\circ} C$ to $T=107^{\circ} C$. (a) Draw a pV-diagram for this process. (b) Calculate the work done by the gas.

A blacksmith cools a 1.20-kg chunk of iron, initially at $650.0^{\circ} \mathrm{C}$, by trickling $15.0^{\circ} \mathrm{C}$ water over it. All of the water boils away, and the iron ends up at $120.0^{\circ} \mathrm{C}$. How much water did the blacksmith trickle over the iron?