3.3 First Law of Thermodynamics

The quantities below represent four different transitions between the same initial and final state. Fill in the blanks.

Why was it necessary to state that the process of the example is quasi-static?

When 1.00 g of ammonia boils at atmospheric pressure and $−33.0 ° \text{C},$ its volume changes from 1.47 to $1130 \left( \text{cm}\right)^{3}$. Its heat of vaporization at this pressure is $1.37 \times 10^{6} \text{J}/\text{kg} .$ What is the change in the internal energy of the ammonia when it vaporizes?

Does adding heat to a system always increase its internal energy?

In an expansion of gas, 500 J of work are done by the gas. If the internal energy of the gas increased by 80 J in the expansion, how much heat does the gas absorb?

A monatomic ideal gas undergoes a quasi-static process that is described by the function $p \left(V\right) = p_{1} + 3 \left(V - V_{1}\right)$, where the pressure and volume are measured in SI units, the starting state is $\left(p_{1} , V_{1}\right)$, and the final state is $\left(p_{2} , V_{2}\right)$. Assume the system consists of n moles of the gas in a container that can exchange heat with the environment and whose volume can change freely. (a) Evaluate the work done by the gas during the change i…