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Standard XII

Chemistry

Activation Energy

If a reaction...

Question

If a reaction, $A + B ⟶ C$ , is exothermic to the extent of $30 k J / m o l$ and the forward reaction has an activation energy of $249 k J / m o l$ , the activation energy for reverse reaction in $k J / m o l$ is:

324

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279

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100

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Solution

The correct option is B $279$
Given that $Δ H = - 30$ kJ/mol......[exothermic reaction]
$Δ H = E_{f} - E_{b}$

$E_{b} = E_{f} - Δ H$

$E_{f} = 249 k J / m o l$

$E_{b} = 249 - (- 30) = 279 k J / m o l$
Option B is correct.

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If a reaction, $A + B \to C$ is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mol, the activation energy for the reverse reaction is (in kJ/mol):

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In an exothermic reaction $A \to B$ , the activation energy of reverse reaction is twice that of forward reaction. If enthalpy of the reaction is -80 kJ $m o l^{- 1}$ , the activation energy of the reverse reaction is :

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If a reaction, A+B⟶C, is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy of 249 kJ/mol, the activation energy for reverse reaction in kJ/mol is:

The correct option is B 279Given that ΔH=−30 kJ/mol......[exothermic reaction]ΔH=Ef−EbEb=Ef−ΔHEf=249kJ/molEb=249−(−30)=279kJ/molOption B is correct.

If a reaction, $A + B ⟶ C$ , is exothermic to the extent of $30 k J / m o l$ and the forward reaction has an activation energy of $249 k J / m o l$ , the activation energy for reverse reaction in $k J / m o l$ is:

The correct option is B $279$
Given that $Δ H = - 30$ kJ/mol......[exothermic reaction]
$Δ H = E_{f} - E_{b}$

$E_{b} = E_{f} - Δ H$

$E_{f} = 249 k J / m o l$

$E_{b} = 249 - (- 30) = 279 k J / m o l$
Option B is correct.