When solid carbon dioxide gas at 1.160 K were put into a rigid 2 L container and the reaction shown below occurred.
C + CO2 <=> 2 CO
As the reaction proceeded, the total pressure in the container was monitored. When equilibrium was reached, some C remained in the container. The results are recored below :
Time in Hours Total Pressure of Gases in atm, in the Container at 1160 K
0 -> 5.00
2 -> 6.26
4 -> 7.09
6 -> 7.75
8 -> 8.37
10 -> 8.37
A) Write the expression for the equilibrium constant, Kp, for the reaction.
B) Calculate the number of moles of CO2 initially placed in the container, assuming the volume of solid carbon is negligible.
C) For the reaction mixture at equilibrium at 1160 K, the partial pressure of CO2 is 1.63 atm. Calculate using the ice table:
pCO pCO2
Initial
Change
Equilibrium
I) The partial pressure of CO
II) The value of the equilibrium constant Kp
D) To another experiment involving the same reaction, a rigid 2 L container initially contained 10 g of C plus CO and CO2, each at 2.00 atm at 1160 K. Predict whether the partial pressure of CO will increase, decrease or remain the same as this system approaches equilibrium.