Heat capacity: Cp and Cv
Chemical Thermodynamics · Chemistry
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2 mol of ideal gas heated 300→350 K at constant pressure (C_P = 29 J/mol·K). Find q and ΔH. Step 1: q_p = nC_P ΔT = 2 × 29 × 50 = 2900 J. Step 2: ΔH = q_p = 2.9 kJ. Step 3: C_V = C_P − R = 29 − 8.314 = 20.7 J/mol·K. Step 4: ΔU = nC_V ΔT = 2 × 20.7 × 50 = 2070 J; difference (830 J) = expansion work. At constant pressure part of heat becomes work — hence C_P > C_V.