A gas in a cylinder is held at a constant pressure of $1.80\times {10}^5$ Pa and is cooled and compressed from $1.70$ m³ to $1.20$ m³. The internal energy of the gas decreases by $1.40\times {10}^5$ J. Does it matter whether the gas is ideal? Why or why not?

Five moles of an ideal monatomic gas with an initial temperature of $127$°C expand and, in the process, absorb $1500$ J of heat and do $2100$ J of work. What is the final temperature of the gas?

A gas in a cylinder expands from a volume of $0.110$ m³ to $0.320$ m³ . Heat flows into the gas just rapidly enough to keep the pressure constant at $1.65\times {10}^5$ Pa during the expansion. The total heat added is $1.15\times {10}^5$ J. Find the work done by the gas.

The $pV$-diagram in Fig. E$19.13$ shows a process $abc$ involving $0.450$ mol of an ideal gas. How much heat had to be added during the process to increase the internal energy of the gas by $15,000$ J?

When water is boiled at a pressure of $2.00$ atm, the heat of vaporization is $2.20\(\times\)10^6$ J/kg and the boiling point is $120$°C. At this pressure, $1.00$ kg of water has a volume of $1.00\(\times\)10^{-3}$ m³, and $1.00$ kg of steam has a volume of $0.824$ m³. Compute the increase in internal energy of the water.

The process $abc$ shown in the $pV$-diagram in Fig. E$19.11$ involves $0.0175$ mol of an ideal gas. What was the lowest temperature the gas reached in this process? Where did it occur?

When water is boiled at a pressure of $2.00$ atm, the heat of vaporization is $2.20\times {10}^6$ J/kg and the boiling point is $120$°C. At this pressure, $1.00$ kg of water has a volume of $1.00\times {10}^{-3}$ m³, and $1.00$ kg of steam has a volume of $0.824$ m³. Compute the work done when $1.00$ kg of steam is formed at this temperature.