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11 Dec 2019
Hydrogen and carbon dioxide can be used to produce carbon monoxide according to the water-gas shift reaction given by: H2 + CO2 = CO + H2O.
If a reaction is set-up initially with n moles each of H2 and CO2 and none of either of the products, CO and H2O, and the variable x represents the fraction of H2 dissociated at equilibrium. Complete the following table in terms of n and x.
H2
CO2
CO
H2O
Total moles
Moles at reaction start
n
n
0
0
2n
Moles at equilibrium
N(1-x)
2n
At T=298 K, the equilibrium constant for this reaction is Kp(298)=10-5. The value of x at 298 K(to a precision of 0.00001)
Hydrogen and carbon dioxide can be used to produce carbon monoxide according to the water-gas shift reaction given by: H2 + CO2 = CO + H2O.
If a reaction is set-up initially with n moles each of H2 and CO2 and none of either of the products, CO and H2O, and the variable x represents the fraction of H2 dissociated at equilibrium. Complete the following table in terms of n and x.
H2 | CO2 | CO | H2O | Total moles | |
Moles at reaction start | n | n | 0 | 0 | 2n |
Moles at equilibrium | N(1-x) | 2n |
At T=298 K, the equilibrium constant for this reaction is Kp(298)=10-5. The value of x at 298 K(to a precision of 0.00001)
Deanna HettingerLv2
13 Dec 2019