If one mole of an ideal gas at P 1 , V 1 is allowed to expand reversibly and isothermally ( A to B ) its pressure is reduced to one-half of the original pressure (see figure). This is followed by a constant volume cooling till its pressure is reduced to one-fourth of the initial value B → C …

Question

If one mole of an ideal gas at P 1 , V 1 is allowed to expand reversibly and isothermally ( A to B ) its pressure is reduced to one-half of the original pressure (see figure). This is followed by a constant volume cooling till its pressure is reduced to one-fourth of the initial value B &#8594; C . Then it is restored to its initial state by a reversible adiabatic compression ( C to A ). The net workdone by the gas is equal to:

Aicharya · Accepted Answer

A - B = isothermal process W A B = P 1 V 1 &#160; ln 2 V 1 &#160; V 1 = P 1 V 1 ln 2 B - C &#8594; Isochoric process W B C = 0 C - A &#8594; Adiabatic process W C A = P 1 V 1 - P 1 4 &#215; 2 V 1 1 - &#947; = P 1 V 1 1 - 1 2 1 - &#947; = P 1 V 1 2 1 - &#947; W net = W A B + W B C + W C A &#160;&#160; P 1 V 1 = R T = P 1 V 1 &#160; ln 2 + 0 + P 1 V 1 2 1 - &#947; W net = R T &#160; ln 2 - 1 2 &#947; - 1

If one mole of an ideal gas at P 1 , V 1 is allowed to expand reversibly and isothermally ( A to B ) its…

Solution