You and your lab partner are studying the rate of a reaction, A + B --> C. You m
ID: 884094 • Letter: Y
Question
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:
(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] = 0.4 and [B] = 0.7
[A] = 0.2 and [B] = 1.4
[A] = 1.0 and [B] = 0.7
[A] = 0.8 and [B] = 0.7
[A] = 0.6 and [B] = 0.7
[A] = 0.4 and [B] = 2.1
[A] = 0.4 and [B] = 1.4
[A] = 0.2 and [B] = 2.1
(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 doubling the concentration of C increases the rate by a factor of 8. 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)?
Explanation / Answer
a) [A] = 0.2 and [B] = 1.4
[A] = 0.2 and [B] = 2.1
[A] = 0.4 and [B] = 1.4
[A] = 0.4 and [B] = 2.1
b) Rate = k[A][C]3
c) rate decreased by 4 times
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