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
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
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Collision Theory concept. You can view video lessons to learn Collision Theory. Or if you need more Collision Theory practice, you can also practice Collision Theory practice problems.