at you 16:17 I know the question asked for change in S of the surroundings but I was wondering if we should always use change in S of the surroundings when looking at the chart. Or does it depend on the question?
If a spontaneous process is endothermic, that would mean delta H needs to be positive. That said, how would that affect the entropy of the surroundings? Decreasing?
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Having engineering thermodynamics tomorrow. Wish I found this on time!!!
at you 16:17 I know the question asked for change in S of the surroundings but I was wondering if we should always use change in S of the surroundings when looking at the chart. Or does it depend on the question?
Thank you so much. That helped a lot!!!
You're welcome!
Thanks that helped a lot
If a spontaneous process is endothermic, that would mean delta H needs to be positive. That said, how would that affect the entropy of the surroundings? Decreasing?
All spontaneous processes are not exothermic, because it is the Gibbs Free energy that determines spontaneity, not the enthalpy.
On my calculator for the advanced thermochemistry problem I did not get -7.32•10^7 instead I got -1.65•10^6. How did you get your answer?
You r right.i too got ur answer
That's because she accidently divided the two numbers. However, you are supposed to mutilply so you were correct.
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Thank you for the help! :)
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3:15
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