Question

We now consider three moles of ideal gas at the same initial state (3.0 L at 273 K). This time, we will first perform an isobaric compression, then an isothermal expansion to bring the gas to the final state with the same volume of 3.0 L, and at temperature 110 K. Hint (a) How much work (in J) is done on the gas during the isobaric compression?

Answer 1

Answer:

The work was done on the gas during the isobaric compression is: 4065.78 (Joules)

Explanation:

We need to use the ideal gas law $PV=nRT$ where P is the pressure, V is the volume, n the moles number, T the temperature and R is the ideal gas constante which value is:$8.314472(\frac{Joules}{K*mol} )$, replacing the values for the first state, we get: $P_{1} V_{1}=nRT_{1}=3*8.314472*273=6809.55(Joules)$ and the second state is:$P_{2} V_{2}=nRT_{2}=3*8.314472*110=2743.78(Joules)$, but we need to know what was the work was done on the gas during the isobaric compression that will be the difference between first and second state's energy so: 6809.55-2743.78=4065.78(Joules).