Question

A gaseous reaction mixture contains \(0.30 \mathrm{~atm} \mathrm{SO}_{2}\), \(0.16 \mathrm{~atm} \mathrm{Cl}_{2},\) and \(0.50 \mathrm{~atm} \mathrm{SO}_{2} \mathrm{Cl}_{2}\) in a \(2.0-\mathrm{L}\) container. \(K=0.011\) for the equilibrium system $$ \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) $$ (a) Is the system at equilibrium? Explain. (b) If it is not at equilibrium, in which direction will the system move to reach equilibrium?

Short answer

(b) If not, in which direction will the reaction proceed to reach equilibrium? a) To determine if the system is at equilibrium, compare the calculated reaction quotient (Q) with the given equilibrium constant (K). If Q = K, the system is at equilibrium. If Q ≠ K, the system is not at equilibrium. b) If the system is not at equilibrium, the direction in which the reaction will proceed depends on the comparison between Q and K. If Q > K, the reaction will move towards the reactants (left). If Q < K, the reaction will move towards the products (right). The reason for the chosen direction is to establish the equilibrium condition where Q = K.

Step-by-step solution

(Step 1: Calculate the reaction quotient (Q))

(Find the reaction quotient Q by dividing the product of the partial pressures of the products by the partial pressure of the reactant:) $$ Q=\frac{[SO_2][Cl_2]}{[SO_2Cl_2]} $$ Substitute the given partial pressures for each component and calculate Q.

(Step 2: Compare Q with K)

(Determine if the system is at equilibrium by comparing the calculated Q with the given equilibrium constant K. If Q = K, the system is at equilibrium. If Q > K, the reaction will move towards the reactants (left). If Q < K, the reaction will move towards the products (right).)

(Step 3: Determine the direction of the reaction)

(Based on the comparison made in Step 2, decide whether the reaction will move towards the reactants or the products to reach equilibrium. Explain the reason for the chosen direction.)

(Step 4: Answer both parts (a) and (b) of the question)

(a) Determine if the system is at equilibrium from the comparison made in Step 2 and provide an explanation. (b) If the system is not at equilibrium, state which direction the reaction will move to reach equilibrium and the reason for the chosen direction.)