The reaction of CH4 in

2CH4(g) ---->/<---- C2H2(g) + 3 H2 (g)

is carried out at a different temperature with an initial concentration of [CH4]=0.087M. At equilibrium, the concentration of H2 is 0.012 M. Find the equilibrium constant at this temperature.

.........2CH4 ==> C2H2 + 3H2

I ......0.087......0......0
C........-2x.......x......3x
E.....0.087-2x.....x......3x

The problem tells you that 3x = 0.012 which allows you to calculate x and 0.087-2x (as well as 3x). Substitute those values into the Keq expression and evaluate Keq.

To find the equilibrium constant (K) at a given temperature, you need to use the equilibrium concentrations of the reactants and products. In this case, the equilibrium concentrations are [CH4] = 0.087 M and [H2] = 0.012 M.

The balanced equation for the reaction is:

2CH4(g) ↔ C2H2(g) + 3H2(g)

The equilibrium constant expression, K, can be written as follows:

K = ([C2H2] * [H2]^3) / [CH4]^2

Substituting in the given equilibrium concentrations:

K = ([C2H2] * (0.012 M)^3) / (0.087 M)^2

Simplifying:

K = ([C2H2] * 0.0001728 M^3) / 0.007569 M^2

K = [C2H2] * 0.022811

Therefore, at the given temperature and equilibrium concentrations, the equilibrium constant (K) is equal to [C2H2] * 0.022811.

To find the equilibrium constant (Kc) for the given reaction, we need to use the concentration values at equilibrium.

The given balanced equation is:
2 CH4(g) ⇌ C2H2(g) + 3 H2(g)

We are given the concentration of methane (CH4) at equilibrium as [CH4] = 0.087 M, and the concentration of hydrogen (H2) at equilibrium as [H2] = 0.012 M.

Now, let's use these concentrations to calculate the equilibrium constant (Kc).

First, we need to set up the expression for Kc using the concentrations of the reactants and products raised to the power of their respective coefficients in the balanced equation.

Kc = [C2H2] * [H2]^3 / [CH4]^2

Substitute the given equilibrium concentrations into the equation:

Kc = [C2H2] * (0.012 M)^3 / (0.087 M)^2

Finally, substitute the values and solve the equation:

Kc = [C2H2] * (0.000012 M^3) / (0.007569 M^2)

Since the concentration of C2H2 (acetylene) is not given, we cannot calculate the exact value of Kc without that information. The equilibrium constant depends on the specific conditions of the reaction.

0.000608