Question

# A gas phase that is at equilibrium with respect to the following reaction at 500 K...

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

Solution:

Step 1: (a)

Here, we have to calculate the equilibrium partial pressure of oxygen.

Given equation

The equilibrium pressure for the equation is given below Given that   We know that,   Again we know = 3.63 x 103

Step 2:

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 Step 3:

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