23.Consider the following equilibrium process at 686 ° C: CO 2 ( g ) + H 2 ( g )

Question

23.Consider the following equilibrium process at 686°C:

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

The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M,

[CO2] = 0.0900 M,

and [H2O] = 0.0420 M.

(a) Calculate Kc for the reaction at 686°C.

________

(b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished?

CO2:

M

H2:

M

CO:

M

H2O:

M

22. The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 ×103 at 527°C:

Calculate the equilibrium partial pressure of all the components, starting with pure phosgene

at 0.760 atm.

The dissociation of molecular iodine into iodine atoms is represented as

I2(g) 2I(g)

At 1000 K, the equilibrium constant Kc for the reaction is 3.80

×

105. Suppose you start with 0.0454 mol of I2 in a 2.29L flask at 1000 K. What are the concentrations of the gases at equilibrium?

What is the equilibrium concentration of I2?



What is the equilibrium concentration of I?

Explanation / Answer

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

Kc = [CO][H2O]/[CO2][H2]

       = 0.058*0.042/0.09*0.043 = 0.63

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

I           0.46      0.043       0.058    0.042

C           -x           -x             +x           +x

E         0.46-x     0.043-x     0.058+ x 0.042+x

    Kc   = [CO][H2O]/[CO2][H2]

    0.63   = (0.058+x)( 0.042+x)/(0.46-x)(0.043-x)

               x = 0.0235

[CO2]   = 0.46-x = 0.46-0.0235 = 0.4365M

[H2]     = 0.043-x = 0.043-0.0235 = 0.0195M

[CO]   = 0.058+ x    = 0.058+0.0235 = 0.0815M

[H2O]   = 0.042+x    = 0.042+0.0235 = 0.0655M

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