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

7247 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How do you determine the shape and bond angle of an ammonia molecule?


In transition metals, where does the formation of colour come from?


The ionic product of water, Kw = 2.93 × 10−15 mol dm−6 at 10 °C. Calculate the pH of a 0.0131 mol dm−3 solution of calcium hydroxide at 10 °C Give your answer to two decimal places.


What is the geometry of a BF3 molecule?


We're here to help

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