2 NH3 (g) ----> N2 9g) + 3 H2 (g)
at equilibrium, [NH3] = 0.0227 M, [N2] = 0.119 M, and [H2] = 0.346 M. Calculate Kc for the reaaction at this temperature
For a general reaction,
aA + bB ---> cC
the equilibrium constant, Kc, is given by
Kc = [products] / [reactants] = (C)^c / ( (A)^a * (B)^b )
The reaction given is: 2 NH3 ---> N2 + 3 H2
Thus,
Kc = (N2) * (H2)^3 / (NH3)^2
Plug in the concentration values given, and solve for Kc. Don't forget the units.
hope this helps~ `u`
To calculate the equilibrium constant, Kc, for the given reaction, we need to use the concentrations of the species at equilibrium.
The balanced chemical equation is:
2 NH3 (g) ----> N2 (g) + 3 H2 (g)
The expression for Kc is:
Kc = ([N2]^n[NH3]^m)/([H2]^p)
Where n, m, and p are the respective coefficients in the balanced chemical equation.
In this case, n = 1, m = 2, and p = 3.
Given the equilibrium concentrations:
[NH3] = 0.0227 M
[N2] = 0.119 M
[H2] = 0.346 M
We can substitute these values into the Kc expression and solve for Kc.
Kc = ([N2]^1[NH3]^2)/([H2]^3)
= (0.119^1)(0.0227^2)/(0.346^3)
Calculating this expression:
Kc = (0.119)(0.0227)^2/(0.346)^3
= 0.000080
Therefore, Kc for the reaction at this temperature is approximately 0.000080.