Statement1 : When the $Δ$ G of a reaction at a given temperature is negative, the reaction occurs spontaneously.
Statement 2: When $Δ$ G is negative, $Δ$ H is also negative.

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

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Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is C
Statement 1 is correct but Statement 2 is not correct.

Statement1 : When the ΔG of a reaction at a given temperature is negative, the reaction occurs spontaneously.
For non spontaneous reaction ΔG is positive. For equilibrium reaction, ΔG is zero.
Statement 2: When ΔG is negative, ΔH may or may not be negative. If ΔH is positive, ΔS has negative value so that TΔS is more negative than ΔH so that ΔG becomes negative.
Statement 1 is correct but Statement 2 is not correct.

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Statement1 : When the ΔG of a reaction at a given temperature is negative, the reaction occurs spontaneously.Statement 2: When ΔG is negative, ΔH is also negative.

Statement1 : When the $Δ$ G of a reaction at a given temperature is negative, the reaction occurs spontaneously.
Statement 2: When $Δ$ G is negative, $Δ$ H is also negative.