Statement 1: A spontaneous reaction is always exothermic.
Statement 2: Exothermic reactions release energy from the system.

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

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Both the 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 E Statement 1 is not correct but Statement 2 is correct.
All Spontaneous processes are not exothermic because it is Gibbs free energy that determines spontaneity, not the enthalpy.
A process is spontaneous even if the Gibbs free energy is negative.
$Δ$ G = $Δ$ H - T $Δ$ S
It is true that Exothermic reactions release energy from the system.

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Statement 1: A spontaneous reaction is always exothermic. Statement 2: Exothermic reactions release energy from the system.

Statement 1: A spontaneous reaction is always exothermic.
Statement 2: Exothermic reactions release energy from the system.