CHAPTER 1: Reaction Kinetics(Revision 1.1 Reaction Rate)

Given the following balanced equation :

2NO(g) + Cl₂(g) → 2NOCl(g)

If the rate of disappearance of Cl₂ is 4.84 x 10^-2 Ms^-1, what is the rate of disappearance of NO?

• 1.45 x 10^-2 Ms^-1

• 2.42 x 10^-2 Ms^-1

• 3.67 x 10^-2 Ms^-1

• 9.68 x 10^-2 Ms^-1

The reaction A + 2B → products was found to have the rate law, k = k[A][B]². Predict by what factor the rate of reaction will increase when the concentration of B is doubled and the concentration of A remained unchanged?

• 2

• 4

• 6

• 8

The overall order for the reaction,

2A + B → C

is one and with respect to B the order is zero. Which of the following statements is true?

• The rate law of the reaction is rate =k[A]²[B]

• The formation of C is double the appearance of A

• The rate of reaction would increase with increasing concentration B

• The half-life of the reaction is independent on the concentration of the reactants

The experimentally determined rate law for the reaction below,

2 NO(g)   +   2 H₂(g)     →     N₂(g)   +   2 H₂O(g)

is rate = k[NO]²[H₂]. If the concentration of H₂ is doubled, predict what will happen to the reaction rate?

• The reaction rate is quadrupled

• The reaction rate is doubled

• The reaction rate is remain the same

• The reaction rate is tripled

The decomposition of dinitrogen pentoxide, N₂O₅ to dinitrogen tetraoxide, N₂O₄ and oxygen gas, O₂ is as follows:

2 N₂O₅(g)     →     2 N₂O₄(g)   +  O₂(g)

The initial concentration of N₂O₅ is 0.9736 M. After 9.30 minutes, its concentration is reduced to 0.9033 M. Calculate the average rate of this reaction in the period of time.

• 1.82 x 10^-3 M min^-1

• 1.72 x 10^-3 M min^-1

• 7.56 x 10^-3 M min^-1

• 7.38 x 10^-3 M min^-1

Which of the following is a unit of rate of reaction?

• s^-1

• Ms^-1

• M

• M^-1s^-1

A possible rate law for a third overall order of a reaction is __________________

• Rate = k [A]²[B]²

• Rate = k [A][B]³

• Rate = k [A]³ [B]

• Rate = k [A]²[B]

What two trials would you use to find the order for B?

• trials 1 and 2

• trials 1 and 3

• trials 2 and 3

For second order reaction, the initial concentration of reactant A is 0.24 M. If the rate constant is 8.1 x 10^-2 M^-1 s^-1, what is the concentration of A after 29 seconds?

• 0.02 M

• 0.15 M

• 0.30 M

• 0.45 M

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.