Statement I : A reaction with a positive $Δ H$ is considered to be exothermic.
Statement II : An exothermic reaction has more heat released than absorbed.

Statement I is false and Statement II is true

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Statement I is true and Statement II is false

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Both statement I and II are correct and Statement II is the correct explanation of Statement I

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Both Statements I and II are correct statements but the Statement II is not the correct explanation of the Statement I

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Solution

The correct option is A Statement I is false and Statement II is true
For an exothermic reaction,
High amount of heat is liberated than absorbed by the system.
$Δ H$ is taken negative.

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Statement I : A reaction with a positive ΔH is considered to be exothermic.Statement II : An exothermic reaction has more heat released than absorbed.

The correct option is A Statement I is false and Statement II is trueFor an exothermic reaction,High amount of heat is liberated than absorbed by the system.ΔH is taken negative.

Statement I : A reaction with a positive $Δ H$ is considered to be exothermic.
Statement II : An exothermic reaction has more heat released than absorbed.

The correct option is A Statement I is false and Statement II is true
For an exothermic reaction,
High amount of heat is liberated than absorbed by the system.
$Δ H$ is taken negative.