In an experiment, 2.00 mol of hydrogen and 3.00 mol of iodine were heated together in a sealed container and allowed to reach equilibrium at a fixed temperature. The container had a fixed volume of 1.00 dm³. At equilibrium, there were 2.40 mol of iodine present in the mixture.
H₂(g) + I₂(g) ⇌ 2HI(g)
What is the value of the equilibrium constant, K_c?

Q: What topic does this question test?

This question tests Equilibria in A-Level Chemistry (syllabus code 9701). It is worth 1 mark.

Q: Which exam paper is this question from?

This question appeared in the Cambridge A-Level Chemistry Feb/Mar 2016 examination, Paper 1 Variant 2 (9701_m16_qp_12.pdf).

Question

In an experiment, 2.00 mol of hydrogen and 3.00 mol of iodine were heated together in a sealed container and allowed to reach equilibrium at a fixed temperature. The container had a fixed volume of 1.00 dm³. At equilibrium, there were 2.40 mol of iodine present in the mixture.
H₂(g) + I₂(g) ⇌ 2HI(g)
What is the value of the equilibrium constant, K_c?

Oracle Prep · Accepted Answer

The correct answer is C: 0.429.

✓ Correct Answer

📋 Examiner Report & Trap Analysis

🎯 Mark Scheme Breakdown

Unlock the Examiner's Analysis

About This A-Level Chemistry Question

Topic

Source

Practice on Oracle Prep

Related Chemistry Questions