The reaction of CH4 is carried out at a different temperature with an initial concentration of [CH4] = 9.3×10−2 M . At equilibrium, the concentration of H2 is 1.6×10−2 M . 2CH4(g)⇌C2H2+3H2(g) . Find the equilibrium constant at this temperature.
2CH4(g) <--------------------> C2H2 + 3H2(g)
9.3 x 10^-2 0 0 ---------------> initial
9.3 x 10^-2 -2x x 3x -----------------> equilibrium
3x = 1.6 x 10^-2
x = 5.33 x 10^-3
equilibrium concentrations :
[CH4] = 9.3 x 10^-2 -2x = 0.0823 M
[C2H2] = x = 5.33 x 10^-3 M
[H2] = 1.6×10−2 M
Keq = [C2H2] [H2]^3 / [CH4]^2
Keq = (5.33 x 10^-3 ) (1.6×10^−2 )^3 / (0.0823)^2
Keq = 3.22 x 10^-6
equilibrium constant Keq = 3.22 x 10^-6
The reaction of CH4 is carried out at a different temperature with an initial concentration of...
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