<Dl> <Dd> Δ S total = Δ S system + Δ S surroundings ≥ 0 (\ displaystyle \ Delta S_ (\ textrm (total)) = \ Delta S_ (\ textrm (system)) + \ Delta S_ (\ textrm (surroundings)) \ geq 0 \,). </Dd> </Dl> <Dd> Δ S total = Δ S system + Δ S surroundings ≥ 0 (\ displaystyle \ Delta S_ (\ textrm (total)) = \ Delta S_ (\ textrm (system)) + \ Delta S_ (\ textrm (surroundings)) \ geq 0 \,). </Dd> <P> This criterion can then be used to explain how it is possible for the entropy of an open or closed system to decrease during a spontaneous process . A decrease in system entropy can only occur spontaneously if the entropy change of the surroundings is both positive in sign and has a larger magnitude than the entropy change of the system: </P> <Dl> <Dd> Δ S surroundings> 0 (\ displaystyle \ Delta S_ (\ textrm (surroundings))> 0) </Dd> </Dl>

What would cause entropy to decrease in a reaction
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