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Summary AQA A-Level Chemistry 1.10 Equilibrium Constant Kp
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  • AQA A Level Chemistry Revision Guide

These are detailed Revision Notes for Topic 1.10 of AQA A-Level Chemistry (Kp). They were written by me using a combination of the textbook and class notes. I will also be uploading the other topics and creating bundles. Topics Included: - Equilibrium constant Kp for homogenous systems

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  • Chapter 19
  • May 8, 2022
  • 1
  • 2021/2022
  • Summary

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  • chem
  • chemistry
  • aqa chem
  • aqa chemistry
  • a level chem
  • a level chemistry
  • aqa a level chem
  • aqa a level chemistry
  • kp

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Equilibrium Constant, Kp
19.1 Equilibrium Constant Kp for Homogeneous Systems:
19.1 Equilibrium constant
- Many reversible reactions take place in the gas phase.
- Gaseous equilibria also obey the equilibrium law, but it is usual to express their Kp for homogeneous
concentrations in a different way using the idea of partial pressure. systems
!"#$% "' ()% *
- The mole fraction of gas A = +"+)# !"#$% "' ()%
- The partial pressure of a gas in a mixture is found by multiplying the mole fraction of that gas by the
total pressure.
- Partial pressure of gas A = mole fraction of A x total pressure
- It is worked out the same way as Kc but using the partial pressures rather than concentrations.
e.g., 1.00 moles of PCl5 vapour are heated to 500K in a sealed vessel. The equilibrium
mixture, at a pressure of 625kPa, contains 0.600 moles of chlorine. Calculate Kp

PCl5 ⇌ PCl3 + Cl2
Initial mol 1.00 0.00 0.00
Change mol -0.600 +0.600 +0.600
Equilibrium mol 0.400 0.600 0.600
Mol fraction 0.25 0.375 0.375
Partial pressure 156.25 234.375 234.375

(𝑃𝐶𝑙- )(𝐶𝑙. ) 234.375 × 234.375
𝐾, = =
(𝑃𝐶𝑙/ ) 156.25
Kc = 352 kPa

- It is affected by Le Chatelier’s principle in the same way as Kc. Increasing the temperature of an
exothermic reaction pushes the equilibrium to the left and decreases Kp

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