Water Gas The water-gas reaction is a source of hydrogen. Passing steam over hot

Question

Water Gas The water-gas reaction is a source of hydrogen. Passing steam over hot carbon produces a mixture of carbon monoxide and hydrogen: H_2O(g)+C(s) CO(g) + H_2(g) The value of K_c for the reaction at 1000 degree C is 3.00 Times 10^-2. Calculate the equilibrium partial pressures of the products and reactants if P_H2O = 0.442 atm and P_co = 5.000 atm at the start of the reaction. Assume that the carbon is in excess. Be careful about rounding your answers in intermediate steps. You should only round the final answer. Determine the equilibrium partial pressures of H_2O, CO, and H_2 after CO and H_2 at 0.077 atm are added to the equilibrium mixture in part a.

Explanation / Answer

H2O(g) + C(s) ---> CO(g) + H2(g)

at equilibrium

kp = kc(RT)^dn

   = 0.03*(0.0821*1273.15)^1 = 3.136

3.136 = (5.244-x)(0.244-x)/(0.275+x)

x= 0.0486

pH2 = 0.244-0.0486 = 0.1954 atm

pCO = 5.244-0.0486 = 5.1954 atm

pH2O = 0.275+0.0486 = 0.3236 atm

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