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(B) For an ideal gas,enthalpy $H$ is a function of temperature only,i.e.,$H = f(T)$.Since the process is isothermal,the change in temperature $\Delta

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enthalpy remains constant but entropy increases

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(B) For an ideal gas,enthalpy $H$ is a function of temperature only,i.e.,$H = f(T)$.Since the process is isothermal,the change in temperature $\Delta T = 0$,therefore $\Delta H = n C_p \Delta T = 0$,which means enthalpy remains constant.For an expansion process,the final volume $V_f$ is greater than the initial volume $V_i$ $(V_f > V_i)$.The change in entropy for an ideal gas is given by $\Delta S = n R \ln(V_f / V_i)$.Since $V_f / V_i > 1$,$\ln(V_f / V_i) > 0$,therefore $\Delta S > 0$,which means entropy increases.

An ideal gas undergoes isothermal expansion at constant pressure. During the process

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