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CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1360...

CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kp=0.0611 at 2000 K
A reaction mixture initially contains a CO partial pressure of 1360 torr and a H2O partial pressure of 1768 torr at 2000 K.

Part A
Calculate the equilibrium partial pressure of CO2 and H2

? torr

Solutions

Expert Solution

For the reaction CO(g)+H2O(g)⇌CO2(g)+H2(g),

Kp = 0.0611 = PCO2 . PH2 /PCO . PH2O

We see the changes in pressure in of the species, as th reaction proceeds

                        CO(g)    +    H2O(g)    ⇌   CO2(g)    +     H2(g)

Initial partial pressure (torr)            1360            1768               0                      0

Change                                           -x                 -x                 x                      x

At equilibrium                             (1360-x)          (1768-x)            x                      x

Put equilibrium partial pressures in expression of Kp

Kp = 0.0611 = x.x / (1360-x). (1768-x)

x2 = 0.0611 (1360-x). (1768-x)

x2 = 0.0611 (2404480 -1360x -1768x + x2)

x2 = (146913.728 -83.096x -108.025x +0.06112x2)

0.9389x2 + 191.121x - 146913.728 = 0

Solve the quadratic equation, find the value of x.

x = 306 torr

PCO2 = PH2 = x = 306 torr

queen_honey_blossom answered 2 years ago
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