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 | 0.8 | 0.8 | |
2 | 1.6 | 0.8 |
(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] = 3.2 and [B] = 0.8
[A] = 0.8 and [B] = 2.4
[A] = 4.0 and [B] = 0.8
[A] = 1.6 and [B] = 0.8
[A] = 0.8 and [B] = 1.6
[A] = 1.6 and [B] = 2.4
[A] = 2.4 and [B] = 0.8
[A] = 1.6 and [B] = 1.6
(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 .
You and your lab partner are studying the rate of a reaction, A + B -->...
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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 1.8 0.9 2 3.6 0.9 (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]...
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