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 1.0 0.1 2 2.0 0.1 (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] = 0.3 [A] = 4.0 and [B] = 0.1 [A] = 2.0 and [B] = 0.1 [A] = 1.0 and [B] = 0.2 [A] = 2.0 and [B] = 0.3 [A] = 2.0 and [B] = 0.2 [A] = 5.0 and [B] = 0.1 [A] = 3.0 and [B] = 0.1
You and your lab partner are studying the
| Experiment | [A] (M) | [B] (M) | Rate (M/s) |
|---|---|---|---|
| 1 | 1.0 | 0.1 | |
| 2 | 2.0 | 0.1 |
(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.
(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.
(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 _______.
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