Question

One mole each of SO, and NO, were combined in a one-

liter container, and the following reaction was allowed to
come to equilibrium.
SO₂(g) + NO₂(g) = SO₂(g) + NO(g)
The equilibrium concentrations were found to be [SO₂] =
[NO₂] = 0.350 M and [SO,] = [NO] = 0.650 M. Calculate Kc
for the reaction.

Answer 1

The equilibrium constant Kc for the reaction is 1.19.

Calculating Kc for the Reaction:

1. Define the equilibrium constant:

Kc is the equilibrium constant for the reaction expressed in terms of molar concentrations.

It is calculated using the formula:

Kc = [Products]^n / [Reactants]^m

where n and m are the stoichiometric coefficients of the products and reactants, respectively.

2. Identify the concentrations:

From the problem statement, we have the equilibrium concentrations of all four species:

[SO₂] = [NO₂] = 0.350 M

[SO₃] = [NO] = 0.650 M

3. Substitute the concentrations into the Kc formula:

The reaction stoichiometry is 1:1:1:1 for SO₂:NO₂:SO₃:NO. Therefore, n = m = 1 for both products and reactants.

Plug in the concentrations:

Kc = ([SO₃] * [NO])^1 / ([SO₂] * [NO₂])^1

Kc = (0.650 * 0.650) / (0.350 * 0.350)

Kc = 1.1907

The equilibrium constant Kc for the reaction is 1.19.

Answer 2

Answer: Kc = 0.5625

Explanation: The equilibrium constant, Kc, can be calculated using the equilibrium concentrations of the reactants and products: Kc = ([SO₂] * [NO]) / ([SO] * [NO₂]) Plugging in the given concentrations: Kc = (0.350 * 0.650) / (0.650 * 0.350) Kc = 0.5625