Two moles of a diatomic ideal gas (vibrations ignored, $R = 8.314 J mo l^{- 1} K^{- 1}$ ) change from $300 K$ , $10.0 L$ to $450 K$ , $25.0 L$ . The entropy change in $J K^{- 1}$ (two decimals) is

Numerical answer type, answer in J/K, tolerance 0.03.

Answer: 32.09 J/K

Δ S = n [C_{V} ln (T_{2} / T_{1}) + R ln (V_{2} / V_{1})] = 2 [2.5 (8.314) ln 1.5 + 8.314 ln 2.5] = 2 [8.428 + 7.618] = 32.091 J K^{- 1}