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given

2CO(g) + O2(g)  2CO2(g)  K = 3.01×1091
C(graphite) + 1/2O2(g)  CO(g)
K = 2.28×1023

What is the equilibrium constant for the following reaction?

C(graphite) + O2(g)  CO2(g)





Feb 4th, 2015

Follow these steps :  2CO (g) + O2 (g) ---->. 2CO2 (g).   call it eq. 1

C (graphite) + 1/2 O2 (g) -----> CO (g)             call it eq.2

C (graphite) + O2 -------> CO2 (g).                  call it eq 3

Now multiply sq. 2 by2 band add to sq. 1

You get 2 C (graphite) + 2 O2 (g) ----->  2CO2

Divide by 2 and you get C (graphite) + O2 -------> CO2

k1 = [CO2]^2/ [CO]^2 [O2].  And k2 = [CO]/ [C graph][O2]^1/2

And 2k2 = [CO]^2/ [Cgr]^2 [O2}

So k overall =. sqrt ( k1 x 2k2)

                    = sqrt ( 3.01 x 10^91 multiplied by 2 x 2.28 10^23

k overall =. sqrt ( 13.7 x 10^ 114)

              = 3.7 x 10^ 57

Answer: equilibrium  constant for eq. 3 = 3.7 x 10 ^ 57



Feb 4th, 2015

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