A mixture of H₂S(g) and CH₄(g) in the mole ratio 2 : 1 was brought to equilibrium at 700 °C and a total pressure of 1 atm. On analysis, the equilibrium mixture was found to contain 9.54 x 10^-3 mol H₂S. The CS₂ present at equilibrium was converted successively to H₂SO₄ and then to BaSO₄ 1.42 x 10^-3 mol BaSO₄; was obtained. Use these data to determine K_p at 700 °C for the reaction below. Assume pressures are expressed in atmospheres.

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2 H₂S(g) + CH₂(g) = CS₂(g) + 4H₂(g) Kp at 700 °C = ?