For an endothermic reaction, where $Δ H$ represents the enthalpy of the reaction in $k J / m o l$ , the minimum value for the energy of activation will be:

less than

Δ H

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zero

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more than

Δ H

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equal to

Δ H

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Solution

The correct option is B more than $Δ H$

$E_{a F R}$ = $Δ H$ + $E_{a B R}$

For endothermic reaction $Δ H$ = positive thus $E_{a F R}$ > $Δ H$

For exothermic reaction $Δ H$ =negative thus can be said.

$Δ E_{a}$ is always grater than or equal to $Δ H .$

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, the minimum value for the energy of activation will be:

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For an endothermic reaction, where ΔH represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be:

The correct option is B more than ΔHEaFR = ΔH +EaBRFor endothermic reaction ΔH= positive thus EaFR > ΔHFor exothermic reaction ΔH=negative thus can be said.ΔEa is always grater than or equal to ΔH.

For an endothermic reaction, where $Δ H$ represents the enthalpy of the reaction in $k J / m o l$ , the minimum value for the energy of activation will be:

The correct option is B more than $Δ H$

$E_{a F R}$ = $Δ H$ + $E_{a B R}$

For endothermic reaction $Δ H$ = positive thus $E_{a F R}$ > $Δ H$

For exothermic reaction $Δ H$ =negative thus can be said.

$Δ E_{a}$ is always grater than or equal to $Δ H .$