An empty cylindrical canister 1.50 m long and 90.0 cm in diameter is to be filled with pure oxygen at $22.0^{\circ} \mathrm{C}$ to store in a space station. To hold as much gas as possible, the absolute pressure of the oxygen will be 21.0 atm. The molar mass of oxygen is 32.0 g/mol. (a) How many moles of oxygen does this canister hold? (b) For someone lifting this canister, by how many kilograms does this gas increase the mass to be lifted?

A U.S. penny has a diameter of 1.9000 cm at $20.0^{\circ} C$. The coin is made of a metal alloy (mostly zinc) for which the coefficient of linear expansion is $2.6 \times 10^{-5} \mathrm{K}^{-1}$. What would its diameter be on a hot day in Death Valley $\left(48.0^{\circ} \mathrm{C}\right)$? On a cold night in the mountains of Greenland $\left(-53^{\circ} C\right)$?

An aluminum tea kettle with mass $1.10 \textrm{ kg}$ and containing $1.80 \textrm{ kg}$ of water is placed on a stove. If no heat is lost to the surroundings, how much heat must be added to raise the temperature from $20.0^{\circ} \mathrm{C}$ to $85.0^{\circ} \mathrm{C}$?

Perfectly rigid containers each hold n moles of ideal gas, one being hydrogen $\left(H_{2}\right)$ and the other being neon (Ne). If it takes 300 J of heat to increase the temperature of the hydrogen by $2.50^{\circ} \mathrm{C}$, by how many degrees will the same amount of heat raise the temperature of the neon?

A 6.00-kg piece of solid copper metal at an initial temperature T is placed with 2.00 kg of ice that is initially at $-20.0^{\circ} \mathrm{C}$. The ice is in an insulated container of negligible mass and no heat is exchanged with the surroundings. After thermal equilibrium is reached, there is 1.20 kg of ice and 0.80 kg of liquid water. What was the initial temperature of the piece of copper?

A diesel engine performs 2200 J of mechanical work and discards 4300 J of heat each cycle. (a) How much heat must be supplied to the engine in each cycle? (b) What is the thermal efficiency of the engine?