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Chemistry-

General

Easy

Question

The favourable conditions for a spontaneous reaction are

T $∆$ S> $∆$ H , $∆$ H = +ve, $∆$ S= +ve
T $∆$ S> $∆$ H , $∆$ H = +ve, $∆$ S= -ve
T $∆$ S= $∆$ H , $∆$ H = +ve, $∆$ S= -ve
T $∆$ S= $∆$ H , $∆$ H = +ve, $∆$ S= +ve

The correct answer is: T $increment$ S> $increment$ H , $increment$ H = +ve, $increment$ S= +ve

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$H subscript left parenthesis a q right parenthesis end subscript superscript plus end superscript plus O H subscript left parenthesis a q right parenthesis end subscript superscript minus end superscript rightwards arrow H subscript 2 end subscript O subscript left parenthesis 1 right parenthesis end subscript semicolon capital delta H equals negative v e$ and $increment$ G= -ve then the reaction is

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$M g S O subscript 4 left parenthesis s right parenthesis end subscript plus a q times rightwards arrow M g S O subscript 4 left parenthesis a q right parenthesis end subscript capital delta H equals negative 84 K blank text cals end text$ , $increment$ H of the reaction is known as

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