Explain why during a spontaneous process the entropy change ofthe system could be negative. (How could the entropy of the systemdecrease for a spontaneous process?)

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Collen VonLv2

17 Dec 2019

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(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ∆S_surr? (c) During a certain reversible process, the surroundings undergo an entropy change, ∆S_surr = –78 J/K. What is the entropy change of the system for this process?

coppertermite386

Which of the following statements is true?
a) In any spontaneous process, the entropy of the system alwaysincreases.
b) All spontaneous processes are exothermic.
c) Any spontaneous process is accompanied by a positive free energychange.
d) In order for a process to be spontaneous, the process must beexothermic and the entropy of the system must increase.
e) None of the statements above are true.

I know the answer is e, but I don't know why the other answers werefalse and was hoping that someone could shine some light as to whya-d are false. Thanks!

plumcat544

Indicate whether each statement is true or false. (a) All spontaneous processes are irreversible. (b) The entropy of the universe increases for spontaneous processes. (c) The change in entropy of the surroundings is equal in magnitude and opposite in sign for the change in entropy of the system, for an irreversible process. (d) The maximum amount of work can be gotten out of a system that undergoes an irreversible process, as compared to a reversible process.