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 1 year ago

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