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
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