## You and your lab partner are studying the rate of a reaction, A + B –>…

You and your lab partner are studying the rate of a reaction, A

+ B –> C. You make measurements of the initial rate under the

following conditions:

Experiment | [A] (M) |
[B] (M) |
Rate (M/s) |
---|---|---|---|

1 | 0.2 | 1.9 | |

2 | 0.4 | 1.9 |

(a) Which of the following reactant concentrations could you use

for experiment 3 in order to determine the rate law, assuming that

the rate law is of the form, Rate = k [A]^{x}

[B]^{y}? Choose all correct possibilities.

[A] = 0.6 and [B] = 1.9

[A] = 0.4 and [B] = 3.8

[A] = 1.0 and [B] = 1.9

[A] = 0.4 and [B] = 5.7

[A] = 0.2 and [B] = 3.8

[A] = 0.4 and [B] = 1.9

[A] = 0.2 and [B] = 5.7

[A] = 0.8 and [B] = 1.9

(b) For a reaction of the form, A + B + C –> Products, the

following observations are made: doubling the concentration of A

increases the rate by a factor of 2, doubling the concentration of

B has no effect on the rate, and doubling the concentration of C

increases the rate by a factor of 2. Select the correct rate law

for this reaction from the choices below.

Rate = k[A][B][C]

Rate = k[A][C]

Rate = k[A]^{2} [C]

Rate = k[A][C]^{2}

Rate = k[A]^{2} [C]^{2}

Rate = k[A]^{3} [C]

Rate = k[A][C]^{3}

(c) By what factor will the rate of the reaction described in part

(b) above change if the concentrations of A, B, and C are all

halved (reduced by a factor of 2)?

The rate will be the original rate multiplied by a factor of

______.