What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if

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Question: What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if at equilibrium [A] = 0.5 M, [B] = 0.2 M, and [C] = 0.3 M?

Options:

0.12
0.30
0.60
1.20

Correct Answer: 0.60

Solution:

Kc = [B][C] / [A]^2 = (0.2)(0.3) / (0.5)^2 = 0.12 / 0.25 = 0.48.

What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if

Practice Questions

What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if at equilibrium [A] = 0.5 M, [B] = 0.2 M, and [C] = 0.3 M?

0.12
0.30
0.60
1.20

Questions & Step-by-Step Solutions

What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if at equilibrium [A] = 0.5 M, [B] = 0.2 M, and [C] = 0.3 M?

Step 1: Write down the balanced chemical equation: 2A ⇌ B + C.
Step 2: Identify the equilibrium concentrations given: [A] = 0.5 M, [B] = 0.2 M, [C] = 0.3 M.
Step 3: Write the formula for the equilibrium constant Kc: Kc = [B][C] / [A]^2.
Step 4: Substitute the equilibrium concentrations into the formula: Kc = (0.2)(0.3) / (0.5)^2.
Step 5: Calculate the numerator: (0.2)(0.3) = 0.06.
Step 6: Calculate the denominator: (0.5)^2 = 0.25.
Step 7: Divide the numerator by the denominator: Kc = 0.06 / 0.25.
Step 8: Perform the division: Kc = 0.24.

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What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if

What’s inside this PDF?

What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if

Practice Questions

Questions & Step-by-Step Solutions

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