Reaction Kinetics part 2

The combustion of ethane (C₂H₆) is represented by the equation:

2C₂H₆(g) + 7O₂(g) -> 4CO₂(g) + 6H₂O(l)

In this reaction:

• the rate of consumption of ethane is seven times faster than the rate of consumption of oxygen.

• the rate of formation of CO₂ equals the rate of formation of water.

• water is formed at a rate equal to two-thirds the rate of formation of CO_2.

• CO₂ is formed twice as fast as ethane is consumed.

What are the units of k for the rate law: Rate = k[A][B]², when the concentration unit is mol/L?

• s^-1

• s

• L mol^-1 s^-1

• L² mol^-2 s^-1

Given: A + 3B -> 2C + D

This reaction is first order with respect to reactant A and second order with respect to reactant B. If the concentration of A is doubled and the concentration of B is halved, the rate of the reaction would _____ by a factor of _____.

• increase, 2

• decrease, 2

• increase, 4

• decrease, 4

• Rate = k[C₂H₅Br]

• .Rate = k[C₂H₅Br]²

• Rate= k[C₂H₅Br][OH^-]

• Rate = k[C₂H₅Br]²[OH^-]

• Rate = k[A][B][C]

• Rate = k[A]²[B]

• Rate = k[B][C]²

• Rate = k[B]²[C]

The rate law for a reaction is rate = k [A][B]²

Which one of the following statements is false?

• If [B] is doubled, the reaction rate will increase by a factor of 4.

• The reaction is second order in B.

• The reaction is first order in A.

• The reaction is second order overall.

Of the following, __________ will provide alternative pathway with lower activation energy for a reaction.

• increasing the concentrations of reactants

• adding a catalyst for the reaction

• raising the temperature of the reaction

• removing products as the reaction proceeds

The rate law of the overall reaction

A + B ->C

is Rate =k[A]².

Which of the following will not increase the rate of the reaction?

• increasing the concentration of reactant A

• increasing the temperature of the reaction

• increasing the concentration of reactant B

• adding a catalyst for the reaction

Which of the following is NOT a property of a catalyst?

• It provide alternative pathway with lower activation energy.

• It increases the rate of both the forward and reverse processes.

• It may be changed at the end of the reaction.

• It causes equilibrium to be reached more rapidly.