SO2 (g) + NO2 (g) ↔ SO3 (g) + NO (g) Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.14 M NO2, 0.12 M SO3 and 0.14 M NO. Which of the following statements is TRUE concerning this system? The reaction will shift in the direction of products. The reaction will shift in the direction of reactants. The reaction quotient will decrease. The equilibrium constant will decrease. The system is at equilibrium.

Question

Virginia Hunt

Chemistry

27 August, 20:12

SO2 (g) + NO2 (g) ↔ SO3 (g) + NO (g) Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.14 M NO2, 0.12 M SO3 and 0.14 M NO. Which of the following statements is TRUE concerning this system? The reaction will shift in the direction of products. The reaction will shift in the direction of reactants. The reaction quotient will decrease. The equilibrium constant will decrease. The system is at equilibrium.

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Answers (1)

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Butterball · Answer 1

The reaction will shift in the direction of products.

Explanation:

Step 1: Data given

A reaction mixture contains:

0.41 M SO2

0.14 M NO2

0.12 M SO3

0.14 M NO

Step 2: The balanced equation

O2 (g) + NO2 (g) ↔ SO3 (g) + NO (g) Kc = 0.33

Step 3: Define the direction of the shift of reaction:

When Q
When Q>K, there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants.

When Q=K, the system is at equilibrium and there is no shift to either the left or the right.

Step 4: Calculate Q

Q = [NO][SO3]/[SO2][NO2]

Q = (0.14 * 0.12) / (0.41*0.14)

Q = 0.0168/0.0574

Q = 0.293

Q
This means there are more reactants than products. Thud, some of the reactants will become products, causing the reaction to shift to the right.

The reaction will shift in the direction of products.