The PV diagram below represents 3.24 mol of an ideal monatomic gas. The gas is i

Question

The PV diagram below represents 3.24 mol of an ideal monatomic gas. The gas is initially at point A. The paths AD and BC represent isothermal changes. If the system is brought to point C along the path ADC, find the following: the initial and final temperatures of the gas initial 60.33 + K final 75.22 (b) the work done by the gas the heat absorbed by the gas kJ

Explanation / Answer

The work done: A Since from A-D-C, the volume of the gas is increase, so the workdone is positive. A-D is isothermal, so A_AD=nRT1*ln(V_D/V_A) and since PV=const soV_D/V_A=P_A/P_D=4 so A_AD=nR60.33ln(4).=2251J D-C, constant pressure , so A_DC=P_D*(V_C-V_D) we have V_D/V_A=4->V_D=16(l)->V_C-V_D=4(l) A_DC=1(atm)*4(l)=400J So A_ADC=2651J The heat absorbed: Since the heat absorbed is to make the gas produced work and tomake its temparature higher so Q=2641 + T*n*(3/2)*R=3241J

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