Define specific heat capacity in terms of the thermal energy needed per unit mass to change temperature.
An ideal gas with mass $0.35\,\text{kg}$ is heated while the pressure stays at $2.0 \times 10^5\,\text{Pa}$, and its internal energy rises by $7600\,\text{J}$. In the process, the volume increases from $0.038\,\text{m}^3$ to $0.063\,\text{m}^3$, while the temperature rises by $56^{\circ}\text{C}$.
Demonstrate that the magnitude of the work done on the gas is $5000\,\text{J}$.
Explain whether the work done on the gas should be positive or negative.
Determine the magnitude of the thermal energy $q$ transferred to the gas.
Calculate the specific heat capacity of the gas for this process. Give a unit in your answer.
The gas in (b) is now heated at constant volume rather than at constant pressure. The gas's increase in internal energy is unchanged from (b). Use the first law of thermodynamics to explain whether the specific heat capacity for this process is less than, the same as, or greater than the answer in (b)(iv).