The activation energy for a simple chemical reaction- A-B is Ea in forward direction- The activation energy for the reverse reaction-

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Standard X

Chemistry

Factors Affecting the Rate of a Chemical Reaction

The activatio...

Question

The activation energy for a simple chemical reaction, $A \to B$ is $E_{a}$ in forward direction. The activation energy for the reverse reaction:

is negative of

E_{a}

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is always less than

E_{a}

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can be less than or more than

E_{a}

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is always double of

E_{a}

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Solution

The correct option is C can be less than or more than $E_{a}$
As we know,
$Δ H = E_{a_{(f)}} - E_{a_{(b)}}$ ; if $Δ H = - v e, E_{a_{(b)}} > E_{a_{(f)}}$
if $Δ H = + v e, E_{a_{(b)}} < E_{a_{(f)}}$

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Similar questions

Q. The activation energy for a simple chemical reaction,

A \to B

E_{a}

in forward direction. The activation energy for reverse reaction.
[CBSE AIPMT 2003]

For an endothermic reaction, energy of activation is $E_{a}$ and enthalpy of reaction is $Δ H$ (both of these in kJ/mol). Minimum value of $E_{a}$ will be:

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 $△ H$ .

Q. In which of the following,

E a

for backward reaction is greater than

E a

for forward reaction?

Q. The temperature dependence of rate constant

(k)

of a chemical reaction is written in terms of Arrhenius equation,

k = A e^{- E_{a} / R T}

. Activation energy

(E_{a})

of the reaction can be calculated by plotting:

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The activation energy for a simple chemical reaction, A→B is Ea in forward direction. The activation energy for the reverse reaction:

The correct option is C can be less than or more than EaAs we know,ΔH=Ea(f)−Ea(b); if ΔH=−ve,Ea(b)>Ea(f)if ΔH=+ve,Ea(b)<Ea(f)

The activation energy for a simple chemical reaction, $A \to B$ is $E_{a}$ in forward direction. The activation energy for the reverse reaction:

The correct option is C can be less than or more than $E_{a}$
As we know,
$Δ H = E_{a_{(f)}} - E_{a_{(b)}}$ ; if $Δ H = - v e, E_{a_{(b)}} > E_{a_{(f)}}$
if $Δ H = + v e, E_{a_{(b)}} < E_{a_{(f)}}$