A gas phase that is at equilibrium with respect to the following reaction at 500 K contains carbon dioxide, carbon monoxide, and oxygen.
2CO2(g) → 2CO(g) + O2(g)
a) Calculate the equilibrium partial pressure of oxygen if the carbon dioxide partial pressure is 0.20 atm and the carbon monoxide partial pressure is 0.40 atm. The ∆G°f values for CO2 and CO at 500 K are -94.389 kcal/mol and -37.140 kcal/mol, respectively.
b) Calculate the total pressure at equilibrium if the mixture contains 3.50 moles of carbon dioxide, 2.00 moles of carbon monoxide, and 2.10 moles of oxygen
Step 1: (a)
Here, we have to calculate the equilibrium partial pressure of oxygen.
The equilibrium pressure for the equation is given below
We know that,
Again we know
= 3.63 x 103
Initially, Partial pressure of CO2 = 0.2 atm
Initially, Partial pressure of CO = 0.4 atm
At equilibrium, Partial pressure of CO2 = (0.2 -2x) atm
Partial pressure of CO = (0.4+2x) atm
Partial pressure of O2 = x atm
Kp = (0.2-2x)2/ x (0.4+2x)
3.63 x 103 = 0.2/0.4x
The equilibrium pressure for oxygen is
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