CHE 1302 Lecture Notes - Lecture 4: Bromine, Rate Equation, Reaction Rate

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20 Dec 2017

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Notice that the rate law is written in terms of reactant concentrations only. From experiment to experiment , both [a] and [b] have changed so we cannot compare these two experiments: we don"t know how much each reactant contributes to the change in rate between and . From experiment to experiment , [b] did not change but [a] has increased by a factor of. Let"s call the reaction rates for these two experiments r2 and r3. Since [a] increased by a factor of 2, we are looking for the rate to increase by a factor of 2m (i. e. , 1, 2, 4, 8, etc ). The ratio of rates is 4. 01 or approximately 4 = 22 and so m = 2. From experiment to experiment , [a] did not change but [b] was increased by a factor of. Let"s call the reaction rates for these two experiments r1 and r2. The ratio of the two rates is: ratio of rates =

Related Questions

[A] = 8.0 and [B] = 1.1

[A] = 4.0 and [B] = 2.2

[A] = 4.0 and [B] = 1.1

[A] = 4.0 and [B] = 3.3

[A] = 2.0 and [B] = 3.3

[A] = 10.0 and [B] = 1.1

[A] = 2.0 and [B] = 2.2

[A] = 6.0 and [B] = 1.1

(b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 3, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 3. 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______

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	0.5	1.2
2	1.0	1.2

(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] = 1.0 and [B] = 3.6

[A] = 1.0 and [B] = 1.2

[A] = 1.5 and [B] = 1.2

[A] = 0.5 and [B] = 3.6

[A] = 0.5 and [B] = 2.4

[A] = 1.0 and [B] = 2.4

[A] = 2.0 and [B] = 1.2

[A] = 2.5 and [B] = 1.2

(b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 9, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 9. 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

You and your lab partner are studying the rate of a reaction, A + B--> C. You make measurements of the initial rate under thefollowing conditions:

Experiment [A] (M) [B] (M) Rate (M/s)
1 0.4 1.9
2 0.8 1.9

(a) Which of the following reactant concentrations could you usefor experiment 3 in order to determine the rate law, assuming thatthe rate law is of the form, Rate = k [A]x [B]y? Choose all correctpossibilities.

[A] = 0.8 and [B] = 5.7
[A] = 0.4 and [B] = 5.7
[A] = 2.0 and [B] = 1.9
[A] = 0.4 and [B] = 3.8
[A] = 0.8 and [B] = 3.8
[A] = 1.6 and [B] = 1.9
[A] = 1.2 and [B] = 1.9
[A] = 0.8 and [B] = 1.9

(b) For a reaction of the form, A + B + C --> Products, thefollowing observations are made: doubling the concentration of Aincreases the rate by a factor of 2, doubling the concentration ofB has no effect on the rate, and tripling the concentration of Cincreases the rate by a factor of 9. Select the correct rate lawfor 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 allhalved (reduced by a factor of 2)?

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

CHE 1302 Lecture Notes - Lecture 4: Bromine, Rate Equation, Reaction Rate

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