ok, so ive been trying to do this problem, but all i get is 1.38 or something like that which isn't the correct answer and it's getting me mad and driving me crazy!!! can you guys help me and do it step by step please?
515. The following reaction is used in the industrial production of hydrogen gas:
CH4(g) + H2O(g) <===> CO(g) + 3H2(g)
The equilibrium constant of this reaction at 298 K (25 C) is 3.896 x 10^-27, but at 1100 K the constant is 3.112 x 10^2.
Suppose the reaction mixture is sampled at 1100 K and found to contain 1.56 M of hydrogen, 3.70 x 10^-2 M of methane, and 8.27 x 10^-1 M of gaseous H2O. What concentration of carbon monoxide would you expect to find?
515. The following reaction is used in the industrial production of hydrogen gas:
CH4(g) + H2O(g) <===> CO(g) + 3H2(g)
The equilibrium constant of this reaction at 298 K (25 C) is 3.896 x 10^-27, but at 1100 K the constant is 3.112 x 10^2.
Suppose the reaction mixture is sampled at 1100 K and found to contain 1.56 M of hydrogen, 3.70 x 10^-2 M of methane, and 8.27 x 10^-1 M of gaseous H2O. What concentration of carbon monoxide would you expect to find?
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I haven't spotted what you're doing wrong, but here is how to get the answer.
Keq = [CO][H2]^3 / [CH4][H2O]
Solve for [CO] and get
[CO] = Keq[CH4][H2O] / [H2]^3
[CO] = (3.112 x 10^2)(3.7 x 10^-2)(8.27 x 10^-1) / (1.56)^3
[CO] = 2.51
Keq = [CO][H2]^3 / [CH4][H2O]
Solve for [CO] and get
[CO] = Keq[CH4][H2O] / [H2]^3
[CO] = (3.112 x 10^2)(3.7 x 10^-2)(8.27 x 10^-1) / (1.56)^3
[CO] = 2.51