State what are the equilibrium partial pressures of each gas

Reference no: EM13265992

A 125.4 g quantity of water and an equal molar amount of carbon monoxide were place in an empty 10.0L vessel, and the mixture was heated to 700 K. At equilibrium, the partial pressure of CO was 9.8 atm. The reaction is

CO(g) + H2O(g) === CO2(g) + H2(g)
I calculated Kp at 700 K to be 9.50.

b) An additional 31.4 g of water was added to the reaction vessel, and a new state of equilibrium was achieved. What are the equilibrium partial pressures of each gas in the mixture?
i got 6.86,16.9,33.1,33.1

c. What is the concentration of H2 in molecules/cm^3

Reference no: EM13265992

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