Assertion :All combustion reactions are exothermic. Reason: Enthalpies of products are greater than enthalpies of reactants $(\sum v_{p} Δ_{f} H (P) > \sum v_{R} Δ_{f} H (R))$

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is C Assertion is correct but Reason is incorrect
All combustion reactions are exothermic as they release heat and for all exothermic reactions, enthalpies of products are lesser than enthalpies of reactants $(\sum v_{p} Δ_{f} H (P) < \sum v_{R} Δ_{f} H (R))$

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Similar questions

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Assertion :All combustion reactions are exothermic. Reason: Enthalpies of products are greater than enthalpies of reactants (∑vpΔfH(P)>∑vRΔfH(R))

The correct option is C Assertion is correct but Reason is incorrectAll combustion reactions are exothermic as they release heat and for all exothermic reactions, enthalpies of products are lesser than enthalpies of reactants (∑vpΔfH(P)<∑vRΔfH(R))

Assertion :All combustion reactions are exothermic. Reason: Enthalpies of products are greater than enthalpies of reactants $(\sum v_{p} Δ_{f} H (P) > \sum v_{R} Δ_{f} H (R))$

The correct option is C Assertion is correct but Reason is incorrect
All combustion reactions are exothermic as they release heat and for all exothermic reactions, enthalpies of products are lesser than enthalpies of reactants $(\sum v_{p} Δ_{f} H (P) < \sum v_{R} Δ_{f} H (R))$