For a reaction $A + B ⇆ C + D$ , if the activation energy of backward reaction is more than that of forward reaction, the forward reaction is :

endothermic

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exothermic

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reaction need not necessarily involve heat changes

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cannot predicted

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Solution

The correct option is B exothermic
The minimum energy requirement that must be met for a chemical reaction to occur is called the activation energy. The activation energy of the reverse reaction is greater than the activation energy of the forward reaction, shows that forward reaction is exothermic as it need less energy to proceed.

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Similar questions

Q. If the reactants are at a higher energy level than products, the reaction is exothermic. The activation energy of a forward reaction is less than that of the backward reaction. That means, the energy required for breaking of bonds is less than the energy released during formation of bonds. In case of an endothermic reaction, the activation energy of the forward reaction is more than that of backward reaction.

Q. Assertion :Activation energy of forward reaction is greater than that of backward reaction. Reason: The reaction considered is endothermic in forward direction.

Consider figure and mark the correct option.

(a) Activation energy of forward reaction is $E_{1}$ + $E_{2}$ and product is less stable than reactant

(b) Activation energy of forward reaction is $E_{1}$ + $E_{2}$ and product is more stable than reactant

(c) Activation energy of both forward and backward reaction is $E_{1}$ + $E_{2}$ and reactant is more stable than product

(d) Activation energy of backward reaction is $E_{1}$ and product is more stable than reactant

Q. For a reaction,

A + B \to C + D; Δ H = - 20 K J m o l e^{- 1}

The activation energy for the forward reaction is 85

k J

. Then the activation energy for the backward reaction is:

For the reaction $A + B \to C + D Δ H = - 20 k J m o l^{- 1}$ . The activation energy of the forward reaction is $85 k J m o l^{- 1}$ . The activation energy for backward reaction is

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For a reaction A+B⇆C+D, if the activation energy of backward reaction is more than that of forward reaction, the forward reaction is :

For a reaction $A + B ⇆ C + D$ , if the activation energy of backward reaction is more than that of forward reaction, the forward reaction is :