The following reaction: SO2 (g) <====> SO3 (g) + NO (g) having reached a state of equilibrium, was found to contain 0.40 M SO3, 0.30 M NO, 0.15 M NO2, and 0.20 M SO2. Calculate the equilibrium constant for this reaction. Describe the direction ad extent of a reaction.

SO2 (g) <====> SO3 (g) + NO (g)

C'mon now. You're a better chemist than I if you can get NO on the right side and there is no hint of N on the left side. You can't get something from nothing.

It's rather obvious to me that the equation should be

SO2 (g) + NO2 <====> SO3 (g) + NO (g)
Write the equilibrium expression for the equation. plug in the values given in the problem and solve for K. If K > 1 the extent of the equilibrium is to the right; if K < 0 the equilibrium is to the left.

SO2 (g) <====> SO3 (g) + NO (g)

We have a problem here. You must have omitted something on the left.

@DrBob222 I don't believe so Sir, that's how the question was given to me.

@DrBob222 Sorry Sir, you're right that makes more sense. Thank you for your help

To calculate the equilibrium constant for this reaction, we first need to write the balanced equation:

SO2 (g) + NO (g) ⇌ SO3 (g) + NO2 (g)

The equilibrium constant, denoted as K, is calculated using the concentrations of the reactants and products at equilibrium. The general formula for the equilibrium constant is:

K = [C]^c [D]^d / [A]^a [B]^b

Where [A], [B], [C], and [D] represent the concentrations of the species involved in the reaction, and a, b, c, and d are the stoichiometric coefficients of the balanced equation.

Given that the concentrations at equilibrium are:
[SO3] = 0.40 M
[NO] = 0.30 M
[NO2] = 0.15 M
[SO2] = 0.20 M

The stoichiometric coefficients for this balanced reaction are:
a = 1 (SO2)
b = 1 (NO)
c = 1 (SO3)
d = 1 (NO2)

Now we can substitute the concentrations and stoichiometric coefficients into the equilibrium constant equation:

K = [SO3]^c [NO2]^d / [SO2]^a [NO]^b

K = (0.40)^1 (0.15)^1 / (0.20)^1 (0.30)^1

K = 0.06 / 0.06

K = 1

Therefore, the equilibrium constant for this reaction is 1.

Now, let's describe the direction and extent of the reaction based on the concentrations given.

At equilibrium, the concentrations of reactants and products do not change. From the given concentrations, we can see that the concentration of SO3 is higher than the initial concentration of SO2 (0.40 M > 0.20 M). This suggests that the forward reaction (formation of SO3) occurs and is favored at equilibrium.

Additionally, the presence of NO2 (0.15 M) suggests that the reverse reaction (formation of NO2) also occurs, as it is a product of the forward reaction.

The concentrations of reactants and products at equilibrium provide insight into the direction and extent of the reaction.