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In: Chemistry

Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO...

Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. What is the equilibrium concentration of [CO], [H2O], [CO2], and [H2]

Solutions

Expert Solution

Answer – We are given, reaction - CO(g)+H2O(g) <-----> CO2(g)+H2(g)

Kc = 102 , [CO] = 0.135 M, [H2O] = 0.135 M

We need to put the ICE chart

      CO(g)+H2O(g) <-----> CO2(g)+H2(g)

I    0.135      0.135            0            0

C     -x            -x             +x         +x

E 0.135-x   0.135-x         +x        +x

We know, Kc = [CO2(g)] [H2(g)] / [CO(g)] [H2O(g)]

102 = x *x / (0.135-x) (0.135-x)

So, 102[(0.135-x) (0.135-x)] = x2

102( x2-0.27x+0.0182) =x2

102x2 -27.54x + 1.86 = x2

101x2 -27.54x + 1.86 = 0

Using the quadratic equation

x = 0.123 M

so equilibrium concentration

[CO(g)] =0.135-x

              = 0.135-0.123

              = 0.012 M

[H2O(g)] =0.135-x

              = 0.135-0.123

              = 0.012 M

[CO2(g)] = x = 0.123 M

[H2(g)] = x = 0.123 M

queen_honey_blossom answered 1 year ago
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