You and your lab partner are studying the rate of a reaction, A + B --> C. You m
ID: 1024016 • 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] = 0.5 and [B] = 3.6
[A] = 0.5 and [B] = 5.4
[A] = 1.0 and [B] = 5.4
[A] = 2.0 and [B] = 1.8
[A] = 1.0 and [B] = 1.8
[A] = 1.0 and [B] = 3.6
[A] = 1.5 and [B] = 1.8
[A] = 2.5 and [B] = 1.8
(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 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)? The rate will be the original rate multiplied by a factor of _____ .
experiment [A] Molarity [B] Molarity 1 0.5 1.8 2 1.0 1.8Explanation / Answer
Doubling the concentration of A increases the rate by a factor of 2,So A power is one. Doubling the concentration of B has no effect on the rate,the power of B is zero and doubling the concentration of C increases the rate by a factor of 8. The power of C is 3
B. Rate = k[A][C]3
C. Rate = k[A][C]3
Rate = k[A][C]3
= K1/2[A] *(1/2)3 [C]3
= K[A][C]3 /16
16* Rate = K[A][C]3
16 time
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