Question

An endothermic reaction could be non-spontaneous if the change in enthalpy is less positive than the product of the -TdeltaS is negative? Is this true or false? I am confused.

Answer 1

False, if -TdeltaS is more negative than deltaH is positive, that means deltaH - TdeltaS should be a negative number. |deltaH| < |-TdeltaS|. Therefore, the reaction must be spontaneous. I hope I understood your question correctly

Answer 2

When ΔS is positive and ΔH is negative, a process is always spontaneous

When ΔS is positive and ΔH is positive, a process is spontaneous at high temperatures, where exothermicity plays a small role in the balance.

When ΔS is negative and ΔH is negative, a process is spontaneous at low temperatures, where exothermicity is important.

When ΔS is negative and ΔH is positive, a process is not spontaneous at any temperature, but the reverse process is spontaneous.

Answer 3

so is this true or false?

Answer 4

I find the wording of this question so confusing, I am not sure what is the correct answer.