You are Here: Home

Equilibrium question?

Announcements Posted on
TSR's new app is coming! Sign up here to try it first >> 17-10-2016

1. What does the delta temp mean? Does it mean the forward reaction is exothermic.

I'll take it as if it does, so if the temp increases then wouldn't the equilibrium shift towards the exothermic reaction(which is the forward reaction). So equilibrium shifts toward the left. So more products are formed, as its an exothermic reaction which reduces the temperature .
2. Hi Questioness

You are right when you say the delta value is showing that the forward reaction is exothermic, this is because it is a negative enthalpy value. Unfortunately you have confused yourself afterwards.

The forward reaction is exothermic which means gives out heat. If we increase the temperature of the system this will cause the equilibrium to shift to the side which would counteract this temperature increase, which would be to the left (or the reactants) because this is the ENDOTHERMIC side.

I hope that helps

Alex
3. (Original post by ajsullivan)
Hi Questioness

You are right when you say the delta value is showing that the forward reaction is exothermic, this is because it is a negative enthalpy value. Unfortunately you have confused yourself afterwards.

The forward reaction is exothermic which means gives out heat. If we increase the temperature of the system this will cause the equilibrium to shift to the side which would counteract this temperature increase, which would be to the left (or the reactants) because this is the ENDOTHERMIC side.

I hope that helps

Alex
How would the endothermic counteract and increasing temperature. Endothermic reactions give out heat so that would further increase the temperature?
4. No, your making the same mistake again. EXOthermic means give out heat, ENDOthermic means taking in heat. Read my explanation again reminding yourself off exo and endo.
5. (Original post by Questioness)

What does the delta temp mean? Does it mean the forward reaction is exothermic.

I'll take it as if it does, so if the temp increases then wouldn't the equilibrium shift towards the exothermic reaction(which is the forward reaction). So equilibrium shifts toward the left. So more products are formed, as its an exothermic reaction which reduces the temperature .
Firstly, this is an exothermic reaction. we know that because the enthalpy change for the reaction is a negative value.
In an exothermic reaction, when temperature is increased, the equilibrium shifts to the left and more reactants are formed.
6. Le Chatelier's principle states that when the rate of equilibrium is subjected to a change, the position of the equilibrium will shift to minimise the change. Here, you have been given a negative enthalpy value, meaning that the reaction is exothermic(moving to the right). Therefore, increasing the temperature means that the molecules will move to minimise the change by absorbing energy (endothermic), which shifts to the left.

Register

Thanks for posting! You just need to create an account in order to submit the post
1. this can't be left blank
2. this can't be left blank
3. this can't be left blank

6 characters or longer with both numbers and letters is safer

4. this can't be left empty
1. Oops, you need to agree to our Ts&Cs to register

Updated: April 27, 2016
TSR Support Team

We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out.

This forum is supported by:
Today on TSR

How does exam reform affect you?

From GCSE to A level, it's all changing

Who would you like to thank?

Poll
Study resources

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.