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For a spontaneous process at room temperature \mathrm{( 298 \mathrm{~K})}, which of the following statements is true regarding the entropy change \mathrm{(\Delta S)} and the surroundings?

Option: 1

\mathrm{\Delta S } of the system and surroundings both increase. 


Option: 2

\mathrm{\Delta S} of the system and surroundings both decrease. 


Option: 3

\mathrm{\Delta S} of the system decreases, while \mathrm{\Delta S} of the surroundings increases.


Option: 4

\mathrm{\Delta S} of the system increases, while \mathrm{\Delta S} of the surroundings decreases.


Answers (1)

best_answer

A spontaneous process is characterized by an overall increase in the total entropy of the universe

\mathrm{\left(\Delta S_{\text {total }}=\Delta S_{\text {system }}+\Delta S_{\text {surroundings }}>0\right).}

At room temperature, a process is spontaneous when

\mathrm{\Delta G<0.}

In terms of entropy, this means that \mathrm{ \Delta S_{\text {total }}>0}, which implies that the entropy of the system and surroundings both increase. Therefore, the correct answer is:
A) \mathrm{ \Delta S} of the system and surroundings both increase.

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