An endothermic reaction could be non-spontaneous if the change in enthalpy is less positive than the product of −TΔS is negative.

True or False

Question

An endothermic reaction could be non-spontaneous if the change in enthalpy is less positive than the product of −TΔS is negative.

True or False

aaronq · Answer

what is the condition for spontaneity?

anonymous · Answer

I have no idea

aaronq · Answer

the change in Gibbs free energy (dG) has to be negative for a reaction to be spontaneous.

$$\Delta G =\Delta H-T \Delta S$$

aaronq · Answer

the question is worded funny, it's basically saying that if dH is a lesser value (but positive) than -TdS, then the reaction is spontaneous (dG is negative).

cool?

aaronq · Answer

it's easier to see on a number line:|dw:1375227083716:dw|

anonymous · Answer

and when its negative you get a spontaneous reaction

anonymous · Answer

so it is false!

aaronq · Answer

it's true, because they're saying that if dH is less positive (meaning closer to zero, which is a smaller value) than -TdS is negative (meaning a greater value than dH but negative) dG will be less than zero.

it's really d u m b wording

anonymous · Answer

ok I think I get it now! Thanks!!

aaronq · Answer

no problem, dude !  try looking at it with a number line, it'll make more sense