What's the problem? Substitute into K expression and solve for K.
K = (NCl3)^2/(N2)(Cl2)^3
N2(g) + 3 Cl2(g) 2 NCl3(g)
It is found that [NCl3(g)] = 1.9 10-1 M, [N2(g)] = 1.4 10-3 M, and [Cl2(g)] = 4.3 10-4 M. Calculate K for the reaction at this temperature.
K = (NCl3)^2/(N2)(Cl2)^3
The expression for the equilibrium constant (K) is defined as the product of the concentrations of the products raised to their respective stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their respective stoichiometric coefficients.
In this reaction, the stoichiometric coefficients are 1 for N2, 3 for Cl2, and 2 for NCl3. So, applying that to the expression, we get:
K = ([NCl3(g)]^2) / ([N2(g)][Cl2(g)]^3)
Now let's plug in the given values we have:
K = (1.9x10^-1 M)^2 / (1.4x10^-3 M)(4.3x10^-4 M)^3
After doing some calculations, the answer should be approximately K = 3.5x10^5.
So, K = 3.5x10^5 is the equilibrium constant for the reaction at this temperature.
Hope that puts a smile on your face!
The balanced chemical equation is: N2(g) + 3 Cl2(g) β 2 NCl3(g)
From the given analysis, we have the following concentrations:
[N2(g)] = 1.4 Γ 10^(-3) M
[Cl2(g)] = 4.3 Γ 10^(-4) M
[NCl3(g)] = 1.9 Γ 10^(-1) M
First, let's set up the expression for K:
K = [NCl3(g)] / ([N2(g)] * [Cl2(g)]^3)
Now substitute the concentrations into the expression to find the value of K:
K = (1.9 Γ 10^(-1)) / ((1.4 Γ 10^(-3)) * (4.3 Γ 10^(-4))^3)
Calculating this expression will give you the value of K for the reaction at the given temperature.
[NCl3(g)] = 1.9 Γ 10^(-1) M
[N2(g)] = 1.4 Γ 10^(-3) M
[Cl2(g)] = 4.3 Γ 10^(-4) M
The balanced equation for the reaction is:
N2(g) + 3 Cl2(g) β 2 NCl3(g)
The equilibrium constant expression (K) for this reaction is:
K = ([NCl3(g)])^2 / ([N2(g)] Γ ([Cl2(g)]^3))
Substituting the given concentrations into the equation, we get:
K = (1.9 Γ 10^(-1))^2 / (1.4 Γ 10^(-3) Γ (4.3 Γ 10^(-4))^3)
Simplifying the expression, we have:
K = (3.61 Γ 10^(-2)) / (9.67 Γ 10^(-16))
Dividing the numerator by the denominator, we get:
K = 3.73 Γ 10^13
Therefore, the equilibrium constant (K) for the reaction at the given temperature is 3.73 Γ 10^13.