Problem: Which statement(s) about collision theory is(are) correct?I. Reaction rates are proportional to the number of collisions/secII. Reaction rates increase as the concentrations of reactants increase because the effectiveness of each collision increases.III. Reaction rates increase as temperature increases because the number of collisions/sec increasesA. All statements are correctB. Only statements I and II are correctC. Only statements I and III are correctD. Only statements II and III are correctE. All statements are incorrect

FREE Expert Solution

We’re being asked to determine which of the given statements about gas-phase chemical reactions are true based on the collision theory and Arrhenius concept.


In collision theory, we look at all the different factors that have to be taken into account whenever reactant molecules collide in order for products to be successfully created.


This involves the Arrhenius Equation shown below:

k =A·e-EaRT

A = Frequency Factor
Ea = Energy of Activation
R = Gas Constant = 8.314 J/(mol∙K)
T = Temperature

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Problem Details

Which statement(s) about collision theory is(are) correct?

I. Reaction rates are proportional to the number of collisions/sec

II. Reaction rates increase as the concentrations of reactants increase because the effectiveness of each collision increases.

III. Reaction rates increase as temperature increases because the number of collisions/sec increases

A. All statements are correct

B. Only statements I and II are correct

C. Only statements I and III are correct

D. Only statements II and III are correct

E. All statements are incorrect