For the reaction below, an analysis of an equilibrium mixture is performed at a certain temperature.
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.
What's the problem? Substitute into K expression and solve for K.
K = (NCl3)^2/(N2)(Cl2)^3
Well, well, well! It seems we have some equilibrium analysis going on here. Let's dive right into it and calculate the equilibrium constant, shall we?
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!
To calculate the equilibrium constant (K) for the given reaction, we need to use the concentrations of the reactants and products present in the equilibrium mixture.
The balanced chemical equation is: N2(g) + 3 Cl2(g) ⇌ 2 NCl3(g)
From the given analysis, we have the following concentrations:
[N2(g)] = 1.4 × 10^(-3) M
[Cl2(g)] = 4.3 × 10^(-4) M
[NCl3(g)] = 1.9 × 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 × 10^(-1)) / ((1.4 × 10^(-3)) * (4.3 × 10^(-4))^3)
Calculating this expression will give you the value of K for the reaction at the given temperature.
To calculate the equilibrium constant (K) for the reaction, you need to use the concentrations of the reactants and products at equilibrium. In this case, the given concentrations are:
[NCl3(g)] = 1.9 × 10^(-1) M
[N2(g)] = 1.4 × 10^(-3) M
[Cl2(g)] = 4.3 × 10^(-4) M
The balanced equation for the reaction is:
N2(g) + 3 Cl2(g) ⇌ 2 NCl3(g)
The equilibrium constant expression (K) for this reaction is:
K = ([NCl3(g)])^2 / ([N2(g)] × ([Cl2(g)]^3))
Substituting the given concentrations into the equation, we get:
K = (1.9 × 10^(-1))^2 / (1.4 × 10^(-3) × (4.3 × 10^(-4))^3)
Simplifying the expression, we have:
K = (3.61 × 10^(-2)) / (9.67 × 10^(-16))
Dividing the numerator by the denominator, we get:
K = 3.73 × 10^13
Therefore, the equilibrium constant (K) for the reaction at the given temperature is 3.73 × 10^13.