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For the reaction 2A ⇌ B + C, if the initial concentration of A is 0.5 M and at e

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Question: For the reaction 2A ⇌ B + C, if the initial concentration of A is 0.5 M and at equilibrium, the concentration of B is 0.2 M, what is the equilibrium concentration of A?

Options:

  1. 0.1 M
  2. 0.2 M
  3. 0.3 M
  4. 0.4 M

Correct Answer: 0.4 M

Solution: 

At equilibrium, [A] = 0.5 - 0.2 = 0.3 M.

For the reaction 2A ⇌ B + C, if the initial concentration of A is 0.5 M and at e

Practice Questions

Q1
For the reaction 2A ⇌ B + C, if the initial concentration of A is 0.5 M and at equilibrium, the concentration of B is 0.2 M, what is the equilibrium concentration of A?
  1. 0.1 M
  2. 0.2 M
  3. 0.3 M
  4. 0.4 M

Questions & Step-by-Step Solutions

For the reaction 2A ⇌ B + C, if the initial concentration of A is 0.5 M and at equilibrium, the concentration of B is 0.2 M, what is the equilibrium concentration of A?
  • Step 1: Write down the initial concentration of A, which is 0.5 M.
  • Step 2: Identify the change in concentration of A when the reaction reaches equilibrium. Since 2 moles of A produce 1 mole of B, for every 1 mole of B produced, 2 moles of A are consumed.
  • Step 3: At equilibrium, the concentration of B is given as 0.2 M. This means that 0.2 M of B was produced.
  • Step 4: Calculate how much A was consumed to produce 0.2 M of B. Since 2 moles of A are needed to produce 1 mole of B, we need 2 * 0.2 M = 0.4 M of A.
  • Step 5: Subtract the amount of A consumed from the initial concentration of A. So, [A] at equilibrium = 0.5 M (initial) - 0.4 M (consumed) = 0.1 M.
  • Equilibrium Concentration Calculation – Understanding how to calculate equilibrium concentrations from initial concentrations and changes in concentration during the reaction.
  • Stoichiometry of Reactions – Applying stoichiometric relationships from the balanced chemical equation to determine changes in concentrations.
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