What is the effect of temperature on K(equilibrium constant)?

For this question we need to consider the equation:

ΔStotal = ΔSsystem - ΔH/T

For and exothermic reaction, -ΔH/T is positive. Therefore, as T increases -ΔH/T becomes more negative, ΔStotal becomes less positive/more negative and the position of equilibria moves to the left. This results in K decreasing.

 

For an endothermic reaction, -ΔH/T is negative. Therefore, as T increases, -ΔH/T becomes less negative, ΔStotal becomes less negative/more positive and the position of equilibrium moves to the right. This results in K increasing. 

 

 

OP
Answered by Olivia P. Chemistry tutor

7842 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Explain why alkenes can have stereoisomers


How to answer the question: How does a bicarbonate buffer solution control pH when either an acid or a base is added?


At what temperature does the reaction become feasible? When ΔH = 492.7 kJmol^-1 and ΔS = 542.6 JK^-1mol^-1.


How do mass spectrometers work?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences