Eduqas A Level Chemistry

Eduqas A Level Chemistry PI5.1 Equilibrium Constants Exam Questions

Free Eduqas A Level Chemistry exam questions on PI5.1 Equilibrium Constants, with mark schemes. Covers Kc, Kp, and the effect of conditions on equilibrium constants.

PI5.1 Equilibrium Constants exam questions

1 question pack of real past exam questions with its mark scheme. Answer every question without notes, then mark your answers line by line against the mark scheme.

PI5.1 Equilibrium ConstantsQuestions and mark scheme
A Level Chemistry Flashcards StemUp mark scheme flashcards A Level Chemistry Flashcards Every answer is written in mark scheme wording, so you learn exactly what examiners give marks for. Pick your exam board, then test yourself with the questions on this page. View flashcards

About Eduqas A Level Chemistry PI5.1 Equilibrium Constants

This topic covers quantitative equilibrium.

What you need to know

  • Kc Expression from concentrations at equilibrium, with units.
  • Kp Expression using partial pressures and mole fractions.
  • Temperature Only temperature changes the value of K.
  • Calculations Finding equilibrium amounts from initial values.

Common mistakes in PI5.1 Equilibrium Constants

  • Saying pressure changes Kp.
  • Including solids in Kc expressions for heterogeneous equilibria.
  • Wrong units for K.

Try three PI5.1 Equilibrium Constants exam-style questions

1. Write the Kc expression for H₂ + I₂ ⇌ 2HI. (1 mark)

Show the mark scheme answer

Kc = [HI]² / ([H₂][I₂]).

2. Explain the effect of increasing temperature on Kc for an exothermic reaction. (2 marks)

Show the mark scheme answer

Equilibrium shifts in the endothermic direction to the left (1), so Kc decreases (1).

3. Define mole fraction. (1 mark)

Show the mark scheme answer

Moles of a gas divided by the total moles of gas.

PI5.1 Equilibrium Constants FAQs

What does Equilibrium Constants cover?

Kc and Kp expressions, calculations and the effect of conditions.

Does a catalyst change K?

No, it only speeds up reaching equilibrium.

How are partial pressures found?

Partial pressure = mole fraction x total pressure.