Posted by ChemLover on .
Is the following reaction spontaneous at 25*C?
delta s reaction = -217 J/K*mol
delta H rxn = -1202 KJ
2Mg (s) + O2 (g) -> 2MgO (s)
delta suniverse = delta s system - delta H system / T
i got positive (+) 3.81 x 10 ^ 3 J/K
and my notes says it is spontaneous but i feel like it is non spontaneous
because when delta g is negative and delta h is < tdeltas it should be spontaneous & the opposite of that makes it non spon for an endothermic reaction....i hope this makes sense
my question is why is it spontaneous? thank you in advance
I'm having trouble making sense of it. If DS for the reaction = -217 J/K then why do you have it listed as -217 J/K*mol? So is DS rxn = -217 J or 2*-217 J?
Same kind of question for DH.
DS = -217 J/(K)mol
DH = -1202 KJ -> -1202 x 10^3 J
does this make any sense?