Chemical Kinetics Warm UP

The iodide ion reacts with hypochlorite ion in the following way:

OCl^- + I^- ⟶ OI^- + Cl^-.

This rapid reaction gives the rate data shown. What is the rate law?

• rate = [OCl^-]²[I^-]

• rate = [OCl^-][I^-]²

• rate = [OCl^-][I^-]

• rate = [OCl^-]

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

• doubles

• remains unchanged

• increases by a factor of 4

• is reduced by a factor of 2

Given the following rate law,

rate = k[A]²[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

• [B] must quadruple

• [B] must double

• [B] must be havled

• [B] must be quartered

Which of the following best describes why increasing temperature increase reaction rate?

• Activation energy is reduced.

• Collisions become more frequent.

• Collisions become more energetic.

• Collisions become more frequent and more energetic.

rate = k[A]

The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

• 0.7 s

• 1.4 s

• 2.8 s

• There is not enough information given.