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]

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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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