For the reaction 2NH3(g) 3H2(g) N2(g) at 472oC equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37x10^_8 M. What is the equilibrium constant for the reverse reaction?
Write the equilibrium constant expression and substitute the numbers from the problem. Then solve for Kc
To find the equilibrium constant for the reverse reaction, we can use the equation for the equilibrium constant (K) expression, which is given by the ratio of the products to the reactants, each raised to their stoichiometric coefficients.
For the given reaction:
2NH3(g) + 3H2(g) ⇌ N2(g)
The equilibrium constant expression is:
K = ([N2]^x) / ([NH3]^y * [H2]^z)
x, y, and z are the stoichiometric coefficients of N2, NH3, and H2, respectively.
From the balanced equation, we can see that:
x = 1, y = 2, and z = 3
Plugging in the given equilibrium concentrations:
[N2] = 0.0100 M
[NH3] = 5.37×10^-8 M
[H2] = 0.0200 M
K = ([N2]^x) / ([NH3]^y * [H2]^z)
K = (0.0100^1) / ((5.37×10^-8)^2 * 0.0200^3)
Now we can calculate the equilibrium constant for the reverse reaction of the given reaction.
To find the equilibrium constant (K) for the reverse reaction, we can use the equilibrium concentrations of the reactants and products.
The balanced equation for the reaction is:
2NH3(g) + 3H2(g) ⇌ N2(g)
At equilibrium, the concentrations of the reactants and products can be expressed as follows:
[NH3] = 5.37x10^(-8) M
[H2] = 0.0200 M
[N2] = 0.0100 M
The expression for the equilibrium constant (K) is given by:
K = ([N2]^x * [H2]^y) / ([NH3]^z)
Where x, y, and z are the stoichiometric coefficients for the respective species in the balanced equation.
For the reverse reaction, the equation is:
N2(g) ⇌ 2NH3(g)
Comparing this to the original equation, we can see that the stoichiometric coefficients are reversed.
So, for the reverse reaction:
x = 2 (coefficient of N2)
y = 3 (coefficient of H2)
z = 1 (coefficient of NH3)
Now we can substitute the given equilibrium concentrations and the stoichiometric coefficients back into the equilibrium constant expression:
K(reverse) = ([N2]^x * [H2]^y) / ([NH3]^z)
K(reverse) = ([N2]^(2) * [H2]^(3)) / ([NH3])
K(reverse) = (0.0100^(2) * 0.0200^(3)) / (5.37x10^(-8))
Calculating this expression will give you the equilibrium constant (K) for the reverse reaction.