One of the many reactions which occur when iron ore is smelted in a blast furnace is given below. For this reaction, the equilibrium constant in terms of partial pressures, Kp, is 0.900 at 873 K and 0.396 at 1273 K. Assume the reaction takes place in a vessel containing only product and reactant molecules and that AH and AS do not change with temperature. FeO (s) + CO (g) = Fe (s) + CO2 (g) a) Calculate AH, AG and AS for the reaction at 873 K b) What is the mole fraction of CO2 (g) at 873 K? Include only the gas-phase species in this mole fraction.

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Chemistry

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16 May, 13:43

One of the many reactions which occur when iron ore is smelted in a blast furnace is given below. For this reaction, the equilibrium constant in terms of partial pressures, Kp, is 0.900 at 873 K and 0.396 at 1273 K. Assume the reaction takes place in a vessel containing only product and reactant molecules and that AH and AS do not change with temperature. FeO (s) + CO (g) = Fe (s) + CO2 (g) a) Calculate AH, AG and AS for the reaction at 873 K b) What is the mole fraction of CO2 (g) at 873 K? Include only the gas-phase species in this mole fraction.

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Explanation: AH, AG and AS for the reaction at 873 K

delta G = -RT ln Kp

G = - 8.314 x 873 ln 0.9

= 764.7J/mol

AG = AH-TAS

AH = 764.7 - 8314 (0.9)

Kp = pCO/pCo2

Substitute the values at different temp. Solve simultaneously

Since mole fraction = kp/pCo

Mf = 1.5