Collision Theory Video Lessons

Concept

# Problem: According to collision theory and the Arrhenius concept, which of the following statements about gas-phase chemical reactions are TRUE?i. Reaction rates are proportional to collision frequencyii. The number of effective collisions at a given temperature is related to both the kinetic energy and orientation of the reacting molecules or atomsiii. As the temperature increases, the number of species reaching the transition state of the rate-determining step increasesiv. As the temperature increases, the activation energy of a reaction remains constant. (a) (i) and (ii)(b) (ii) and (iii)(c) (i), (ii), and (iii)(d) (ii), (iii), and (iv)(e) All of the statements are correct

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###### 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:

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

94% (37 ratings)
###### Problem Details

According to collision theory and the Arrhenius concept, which of the following statements about gas-phase chemical reactions are TRUE?

i. Reaction rates are proportional to collision frequency

ii. The number of effective collisions at a given temperature is related to both the kinetic energy and orientation of the reacting molecules or atoms

iii. As the temperature increases, the number of species reaching the transition state of the rate-determining step increases

iv. As the temperature increases, the activation energy of a reaction remains constant.

(a) (i) and (ii)

(b) (ii) and (iii)

(c) (i), (ii), and (iii)

(d) (ii), (iii), and (iv)

(e) All of the statements are correct