1) Compare the heat flow and entropy change of adiabatic expansion of an ideal gas from V_i to V_f (and pressure p_f ) to a two-step process involving isothermal expansion from V_i to V_f , followed by a constant volume depressurization from to pressure p_f

_{---------------------------------------------------------------}

2) For 0.2 mol of ideal monatomic gas, calculate the entropy change for the system and the surroundings for irreversible expansion and heat flow from p₁ = 500,000 Pa, V₁ = 0.001 m3, T₁ = 300 K, to a final state that is in thermal equilibrium with the surroundings at p_f = 24,942 Pa, T_f = 300 K, V_f = 0.02 m3. To do th*is, assume the surroundings is both a thermal reservoir (constant T = T_f with a thermal response time much shorter than the system's) and a mechanical reservoir (constant p_surr = 15,310 with a mechanical response time much shorter than the system's). Hint: one way to do this* is to compare the irreversible expansion to a two-step process in which the first step is an irreversible adiabatic expansion to V_f , and the second step is a constant volume heating to T_f