thermodynamics doubt (chemistry)
can anyone explain this part i highlighted?, cant really seem to grasp the different S(univ) and S(surr) at diff temp and how they are favourable
ive attached the table they're referring to here too
13 Replies
@Dexter
Note for OP
+solved @user to close the thread when your doubt is solved. Mention the user who helped you solve the doubt. This will be added to their stats.S = -q(rev)/T
right??
T cant be negative, and if S is positive then q must be negative
therefore exothermic
sorry sir but im kinda getting confused, how is entropy of universe decreasing if a process is spontaneous?
and if surrounding acts like a heat sink, then how does endothermic spontaneous reaction work?
then the surrounding will act like a heat resorvoir right? as it gives heat to system
did i say dec? i meant increasing 🙂 uni entropy increases for spontaneous processes always.
endothermic takes heat from the surrounding, and if it is spontaneous, ds>0!
like CaCO3 giving you CaO and CO2
you remember ellingham diagram? all processes there are good examples of what you mentioned
right heat sink or reservoir, either way large body, const T, right
oh yeah it makes sense now
thanks for clearing up the conceptual loopholes
+solved @userSir this is based on the idea of 2nd law...the entropy of the universe tends to a maximum..right?
sure
yes
always increases
until
BOOM
and rinse and repeat 😛
Hahahaha...exactly
+solved @champsboy
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