Select the correct statement regarding activation energy:

Activation energy may be greater than the heat of a reaction

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Activation energy is less than the threshold energy

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Rate of reaction is inversely proportional to activation energy

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All of these

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Solution

The correct option is D All of these

Threshold energy is the energy of the transition state that is always greater than the activation energy.

Activation energy is the energy difference between the energy of the transition state and the energy of the reactant.

Heat of a reaction is the energy difference between the product and the reactant,
Heat of the reaction $= E n e r g y o f p r o d u c t - E n e r g y o f r e a c t a n t$

According to Arrhenius equation,
$k = A e^{\frac{- E_{a}}{R T}}$
The rate constant is inversely related to activation energy.

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$H_{2}$ $_{(g)}$ + ${C l}_{2}$ $_{(g)}$ $\to$ 2HCl $_{(g)}$ ... rate = $r_{1}$ ; $D_{2}$ $_{(g)}$ + ${C l}_{2}$ $_{(g)}$ $\to$ 2DCl $_{(g)}$ ... rate = $r_{2}$ ; $r_{1}$ = $r_{2}$ . Then the correct statement among the following is

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. Assertion :The activation energy for an uncatalysed reaction is less than for a catalysed reaction Reason: Negative catalyst increases the activation energy

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]

The activation energy of a catalysed reaction is more than the activation energy of the uncatalysed reaction.

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