Consider the following reaction.
2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)
An equilibrium mixture of this
reaction at a certain temperature was found to have [NO] = 8.1 10-3 M, [H2] = 4.1 10-5 M, [N2] = 5.3 10-2 M, and [H2O] = 2.9 10-3 M. What is the value of the equilibrium constant at this temperature?
i got 4.04e6 is that correct??
I agree.
To determine the value of the equilibrium constant at a given temperature, you need to use the equilibrium concentrations of the reactants and products.
In the given reaction:
2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)
The equilibrium constant expression is given by:
Kc = ([N2] * [H2O]^2) / ([NO]^2 * [H2]^2)
Now, substitute the given equilibrium concentrations into the above expression:
Kc = ((5.3 * 10^-2) * (2.9 * 10^-3)^2) / ((8.1 * 10^-3)^2 * (4.1 * 10^-5)^2)
Calculating this expression will give you the value of the equilibrium constant (Kc).
On evaluating this expression, I found that the value of the equilibrium constant at the given temperature is approximately 3.975 * 10^6, which is different from the value you obtained. Therefore, the value you got, 4.04 * 10^6, is incorrect.
Hence, the correct value of the equilibrium constant at this temperature is approximately 3.975 * 10^6.