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] = 3.6 and [B] = 2.7
[A] = 3.6 and [B] = 1.8
[A] = 1.8 and [B] = 1.8
[A] = 5.4 and [B] = 0.9[
A] = 7.2 and [B] = 0.9
[A] = 1.8 and [B] = 2.7
[A] = 9.0 and [B] = 0.9
[A] = 3.6 and [B] = 0.9
(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 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]
(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
_______
(a) the concentration of B should be different in experiment 3 as that taken in experiment 1&2. The order is calculating by changing concentration of one reactant keeping other constant. Hence correct possibilities are :
[A] = 3.6 and [B] = 2.7
[A] = 3.6 and [B] = 1.8
[A] = 1.8 and [B] = 1.8
[A] = 1.8 and [B] = 2.7
(Answer) .
(b) tripling the concentration of A rate becomes (3)2 = 9 times , hence order with respect to A is 2.
Effect of concentration is zero on rate of reaction w.r.t B, hence order with respect to B is 0.
Tripling the concentration of C rate becomes (3)1 = 3 times , hence order w.r.t C is 1.
Rate = k[A]2[C] (Answer)
(c)
If concentration of A is reduced to half rate becomes (1/4)times and if concentration of C is reduced to half rate becomes (1/2)times. But rate is independent of concentration of B. Hence the rate will be original rate multiplied by a factor of 1/8 . (Answer) .
You and your lab partner are studying the rate of a reaction, A + B -->...
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