One mole of a real gas is subjected to a process from (2 bar, 30 L, 300 K) to (2 bar, 40 L, 500 K).

Question

One mole of a real gas is subjected to a process from (2 bar, 30 L, 300 K) to (2 bar, 40 L, 500 K). The molar heat capacity of gas at constant volume and constant pressure are 25 and 40 J/K- mol, respectively. What is the change in internal energy of the gas in this process?

Accepted Answer

$\Delta H = n.C_{P,m}.\left( T_{2} - T_{1} ight) = 1 	imes 40 	imes (500 - 300) = 8000	ext{ J}$$	herefore\Delta U = \Delta H - P.\Delta V = 8000 - 2(40 - 30) 	imes 100 = 6000	ext{ J}$

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