Question

Which of the following combinations will result in a reaction that is spontaneous at all temperatures?

Negative enthalpy change and negative entropy change
Negative enthalpy change and positive entropy change
Positive enthalpy change and negative entropy change
Positive enthalpy change and positive entropy change
PLS EXPLAIN WHAT EACH MEANS AND THE VARIABLES AND THE EXPLANATION BEHIND IT

Answer 1

from Gibbs Equation,
`\Delta G = \Delta H - T\Delta S`

reaction is spontaneous if $\Delta G$ is negative.

so, first option is not valid at high temperature, ($-h+ts$)

second, is always a spontaneous reaction, ($-h-ts$)

third, is never spontaneous ($+h+ts$)

4th is similar to second, spontaneous at higher temperatures ($+h-ts$)

Answer 2

`\huge\boxed{Option \ 2}`

Step-by-step explanation:

A reaction is spontaneous at all temperatures by the following combinations:

=> A negative enthalpy change (
`\triangle H < 0` )

=> A positive entropy change (
`\triangle S > 0` )

See the attached file for more better understanding!