Question

Based on A(g) + B(g) → C(g) + D(g)

1: A and B must collide to react (rate is proportional to the frequency of collisions (z))
2: A and B collide with an energy greater than some minimum value to result in a reaction
3: Only collisions having the proper orientation of the two reactants can result in a reaction

rate/([A][B]) = k = p x Z x e^-E/RT

p - fraction of collisions having the proper orientation
Z - frequency of collisions

Answer 1

• A and B collide with an energy greater than some minimum value to result in a reaction
• Only collisions having the proper orientation of the two reactants can result in a reaction

In chemistry, the collision theory provides an explanation for the rates at which chemical reactions occur. It suggests that collisions between reacting particles—such as atoms, ions, or molecules—cause chemical reactions. This theory states that these particles must collide with enough energy and in the right direction for a reaction to happen.

Based on the collision theory, the statements 2 and 3 are correct