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Electron Gain Enthalpy

For endotherm...

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For endothermic reaction Ea>delta H (always) Is the same true for exothermic? Or can Ea possibly be greater, less or equal delta H, for exothermic?

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Q. Consider the three statements about reaction energy diagrams and the relative magnitudes of the activation energy,

E_{a}

, and the enthalpy of reaction,

△ H

.
One or more of the statement is true.
Identify the correct statement or combination of statements from the four choices below.

	Statement
I	For an endothermic reaction, the magnitude of $E_{a}$ is always greater than $△ H$ .
II	For an exothermic reaction, the magnitude of $E_{a}$ is always greater than $△ H$ .
III	For an exothermic reaction, adding a catalyst will decrease the magnitude of $△ H$ .

Δ H

for an exothermic reaction is negative and for an endothermic reaction is positive. Reason: Enthalpy is an extensive property.

Q. What is the difference between

Δ

Δ

U? What is the sign of

Δ

H for exothermic and endothermic reactions? Under what circumstances

Δ

Δ

Q. For an exothermic reaction, what is the value of

Δ H

Q. Whether a reaction is endothermic or exothermic can be indicated by:

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