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# For an ideal gas $C_{V}$ and $C_{p}$ are different because of the work W associated with the volume change for a constant-pressure process. To explore the difference between $C_{V}$ and $C_{p}$ for a liquid or a solid, consider the process in which 5.00 mol of ethanol is warmed from 10.0$^{\circ} \mathrm{C}$ to 60.0$^{\circ} \mathrm{C}$ while the applied pressure remains a constant 1.00 atm. The molar mass of ethanol is M=46.1 g/mol. What is the mass of 5.00 mol of ethanol?

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This problem requires a bit of thinking. Since ethanol is not an ideal gas, we cannot use the equation of state of the ideal gas but instead we are going to use general thermodynamic equations. We will first determine the absorbed heat and then, we will determine the work performed due to expansion.

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