How do I calculate the Gibbs free energy change for a reaction when given the entropy change, enthalpy change and the reaction conditions>

deltaG= Gibbs free energy 

deltaG=deltaH - TdeltaS 

If deltaH= 150 kJ/mol and deltaS=2.1 J/mol we must first convert the deltaS into kJ/mol, this is done by multiplying by 10-3 .

So deltaS= 2.1 x 10-3 kJ/mol. If the reaction is done at 25 degrees celcius, we must convert it to Kelvin, by adding 273. This gives 298 K. 

 

So the value of deltaG can be worked out:

 

deltaG= (150 kJ/mol) - (298) x( 2.1x 10-3

deltaG= 149. 4 kJ/mol 

 

AM
Answered by Archit M. Chemistry tutor

9667 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

When vaporised, isotopes of an element can be separated in a mass spectrometer. Name the three processes that occur in a mass spectrometer before the vaporised isotopes can be detected. State how each process is achieved. (6 marks)


What is optical isomerism and how can you distinguish between optical isomers?


Why is a water molecule non-linear?


Explain the trend in boiling points between HF, HCl and HBr.


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 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences