Homework due Monday 10/23/17. Will be checking for the accuracy. Quiz on Monday

Question

Homework due Monday 10/23/17. Will be checking for the accuracy. Quiz on Monday on ideal gases L. A 1.5 mole sample of an ideal gas is expanded from 300K and an Initial volume of 22.5 L to a final volume of 65.0 L Calculate w q, and Au for the following processes.Cpm is 5/2R . For the expansion against a constant pressure of 0.498 atm 4 For the reversible expansion at constant temperature. 2. Two moles of an ideal gas with c, 29.4 K-1mol-1 (independent of temperature) are maintained of 11.35 L is heated reversibly to 373 K at constant volume. Calculate w, q, Au and AH for this process at273K in a volume

Explanation / Answer

U = Cv *  T Given n = 2 mol , Cp = 29.4 J/K/mol , T1 = 273 K, T2 = 373 K , V = 11.35 L

Using Ideal gas equation to find pressure at different temperature at constant volume

P1 = (n*R*T1)/ V = (2 mol*8.314 L kPa/K/mol * 273 K)/ 11.35 L = 399.95 kPa

P2 = (n*R*T1)/ V = (2 mol*8.314 L kPa/K/mol * 373 K)/ 11.35 L = 546.45 kPa

At constant Volume

Therefore, w = 0 and q =0

H = Cp* T = 29.4 J/K/mol *(373-273)K = 2940 J/mol = 2.94 KJ/mol (1KJ= 1000J)

U = Cv *  T

Cv - Cp  = R

Cv =  Cp - R = 29.4 J/K/mol - 8.314 J/K/mol = 21.086 J/K/mol

U = Cv *  T = 21.086 J/K/mol * (373-273)K = 2108.6 J/mol = 2.1086 KJ/mol

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