Which one is correct according to the collision theory of the rate of reaction ?

The threshold energy level is a characterisic of reaction.

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The energy if activation decreases with rise in temperature.

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the energy of adsorbed activated complex is lower than simple activated complex.

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The energy of activated complex (both activated or adsorbed) is higher than reacant or product.

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Solution

The correct options are
A The threshold energy level is a characterisic of reaction.
B The energy if activation decreases with rise in temperature.
C the energy of adsorbed activated complex is lower than simple activated complex.
D The energy of activated complex (both activated or adsorbed) is higher than reacant or product.
According to the collision theory of the rate of reaction
A) The threshold energy level is a characteristics of reaction.
B) The energy if activation decreases with rise in temperature.
C) The energy of absorbed activated complex is lower than simple activated complex.
D) The energy of activated complex (both activated and absorbed) is higher than reactant or product.

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Similar questions

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

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