A mixture of 11.02 mmol of H2S and 5.48 mmol of CH4 is placed in an empty contai

Question

A mixture of 11.02 mmol of H2S and 5.48 mmol of CH4 is placed in an empty container with a platinum catalyst. Catalysts participate in the reaction but are ultimately unchanged, so they do not show up in the balanced chemical reactions. The equilibrium 2H2S(g CH4 4H2(g) CS2(g) is achieved at 700 °C and 762 torr. The reaction mixture is removed from the catalyst and rapidly cooled to room temperature, where the rates of forward and reverse reactions are negligible. Analysis of the equilibrium mixture found 0.711 mmol of CS2. Find KD and AGO for the reaction at 700 °C

Explanation / Answer

2 H2S (g) + CH4 (g) < ------------ > 4 H2 (g) + CS2 (g)

11.02 5.48 0 0 mmol At initial

0.711 0.3255 20.618 5.1545 mmol At equilibrium

Kp = PH24 * PCS2 / PH2S2*PCH4

Kp = (20.618)4 * ( 5.1545 ) / [(0.711)2 * (0.3255)]

Kp = 5.66 * 106

deltaG0 = - R T lnKp

deltaG0 = - 0.008314 * 973.15 * ln(5.66 * 106)

deltaG0 = - 125.8 kJ

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