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Question

A certain reaction is described as $$A + B\rightarrow C$$.
Just because a molecule of $$A$$ collides with a molecule of $$B$$, this does not necessarily result in the formation of a molecule of $$C$$.
Which of the following choices best describes the factor or factors that help to determine whether or not a molecular collision between $$A$$ and $$B$$ will result in the formation of product $$C$$?


A
Molecules of A and B must have the proper orientation when they collide with each other.
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B
Molecules of A and B must have enough energy to overcome the activation energy barrier.
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C
Molecules of A and B must have enough energy to overcome the activation energy barrier and they must have the proper spatial orientation.
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D
For there to be a successful collision, molecules of A and B must be in the gas phase when they collide with each other.
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Solution

The correct option is A Molecules of $$A$$ and $$B$$ must have the proper orientation when they collide with each other.
$$A+B\longrightarrow C$$
 According to collision theory, for a reactant to from product, the reactants must collide each other with proper orientation.
 Therefore, $$(A)$$ is the correct answer.

Chemistry

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