Imagine a reaction A for which the values of ΔH and ΔS are both negative. It is known that the absolute value of ΔS is 3 times smaller than the absolute value of ΔH. For what values of T does reaction A occur spontaneously?

We know that a reaction occurs spontaneously when ΔG<0 and that ΔG=ΔH-TΔS. So, we know that the reaction will be spontaneous when ΔH<TΔS.Its is given that ΔH and ΔS are <0 and that |ΔH|=3*|S|. From this we can conclude that the inequation ΔH<TΔS will be true whenT< 3K. We also have to keep in mind that the temperature can never be lower than the absolute zero (0K) and so, the answer is 0K < T < 3K.

AC
Answered by Andre C. Chemistry tutor

1458 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Briefly describe the nature of three types of intramolecular bonding and two types of intermolecular bonding (drawings encouraged)


Explain why first ionisation energy decreases down a group.


How can you work out, using the changes in oxidation numbers, which compound out of KCl, KBr and KI has the greatest reducing power?


What is the difference between intermolecular and intramolecular bonds.


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