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(C) According to collision theory:$1.$ Not all collisions result in product formation. Only those collisions that possess energy greater than the thre

Vedclass · Accepted Answer

$1-F, 2-F, 3-T$

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(C) According to collision theory:$1.$ Not all collisions result in product formation. Only those collisions that possess energy greater than the threshold energy and have proper orientation are effective,leading to product formation. Thus,statement $1$ is $False$.$2.$ Collisions are only effective if they meet the criteria of threshold energy and proper orientation. Therefore,not all collisions are effective. Thus,statement $2$ is $False$.$3.$ The rate of reaction is directly proportional to the frequency of effective collisions. As the number of total collisions increases,the number of effective collisions generally increases,thereby increasing the rate. Thus,statement $3$ is $True$.

$Step$	$Rate\ Constant\ /\ Activation\ energy$
$Step\ 1$	$k_1, E_{a_1} = 180\ kJ/mol$
$Step\ 2$	$k_2, E_{a_2} = 80\ kJ/mol$
$Step\ 3$	$k_3, E_{a_3} = 50\ kJ/mol$

Find True $(T)$ and False $(F)$ statements among the following:
$1.$ All collisions in a reaction result in the formation of products.
$2.$ All collisions in a reaction are effective.
$3.$ The number of collisions depends on the rate of reaction.

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Find True $(T)$ and False $(F)$ statements among the following:$1.$ All collisions in a reaction result in the formation of products.$2.$ All collisions in a reaction are effective.$3.$ The number of collisions depends on the rate of reaction.