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. 

 

 

Answered by Olivia P. Chemistry tutor

7201 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Explain the reasons for the changes in reactivity of Phenol, Benzene and MethylBenzene


Draw the mechanism for the reaction of an acid chloride with an alcohol to form an ester


By considering the mechanism of the two step reaction of butanone and NaBH4 followed by dilute acid, explain why the product has no effect on plane polarised light.


What is entropy?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences