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The reaction of CH4 is carried out at a different temperature with an initial concentration of...

The reaction of CH4 is carried out at a different temperature with an initial concentration of [CH4] = 9.9×10−2 M . At equilibrium, the concentration of H2 is 2.0×10−2 M

2CH4(g)⇌C2H2(g)+3H2(g)

whats the equilibrium constant

Solutions

Expert Solution

Set up the ICE chart for the reactions as below:

2 CH4 (g) <====> C2H2 (g) + 3 H2 (g)

initial                                     9.9*10-2                       0               0

change                                      -2x                          +x            +3x

equilibrium                      (9.9*10-2 – 2x)                   x              3x

Given the equilibrium concentration of H2 is 2.0*10-2 M, we must have,

3x = 2.0*10-2

===> x = 6.67*10-3

Therefore, [C2H2]eq = 6.67*10-3 M; [CH4] = (9.9*10-2 – 2*6.67*10-3) M = 0.08566 M.

The equilibrium constant is given by

K = [C2H2][H2]3/[CH4]2 = (6.67*10-3)*(2.0*10-2)3/(0.08566)2 = 7.272*10-6 (ans).

queen_honey_blossom answered 3 years ago
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