AIPMT 2009 | Chemical Kinetics Question 46 | Chemistry

In the reaction,
BrO$$_{3(aq)}^ - $$ + 5Br$$_{(aq)}^ - $$ + 6H⁺ $$ \to $$ 3Br_2(l) + 3H₂O_(l).
The rate of appearance of bromine (Br₂) is related to rate of disappearance of bromide ions as

$${{d\left[ {B{r_2}} \right]} \over {dt}} = - {5 \over 3}{{d\left[ {B{r^ - }} \right]} \over {dt}}$$

$${{d\left[ {B{r_2}} \right]} \over {dt}} = {5 \over 3}{{d\left[ {B{r^ - }} \right]} \over {dt}}$$

$${{d\left[ {B{r_2}} \right]} \over {dt}} = {3 \over 5}{{d\left[ {B{r^ - }} \right]} \over {dt}}$$

$${{d\left[ {B{r_2}} \right]} \over {dt}} = - {3 \over 5}{{d\left[ {B{r^ - }} \right]} \over {dt}}$$

AIPMT 2009

MCQ (Single Correct Answer)

-1

For the reaction A + B $$ \to $$ products, it is observed that

(i) on doubling the initial concentration of A only, the rate of reaction is also doubled and
(ii) on doubling the initial concentration of both A and B, there is a change by a factor of 8 in the rate of the reaction.

The rate of this reaction is given by

rate = k[A]² [B]²

rate = k[A] [B]²

rate = k[A] [B]

rate = k[A]² [B]

AIPMT 2009

MCQ (Single Correct Answer)

-1

Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is

0.5 $$ \times $$ 10^$$-$$2 s^$$-$$1

0.5 $$ \times $$ 10^$$-$$3 s^$$-$$1

5.0 $$ \times $$ 10^$$-$$2 s^$$-$$1

5.0 $$ \times $$ 10^$$-$$3 s^$$-$$1.

AIPMT 2008

MCQ (Single Correct Answer)

-1

The bromination of acetone that occurs in acid solution is represented by this equation.
CH₃COCH_3(aq) + Br_2(aq) $$ \to $$
CH₃COCH₂Br(aq) + H⁺_(aq) + Br^$$-$$_(aq)
These kinetic data were obtained for given reaction concentrations.

Initial concentrations, M
[CH₃COCH₃	[Br₂]	[H⁺]
0.30	0.05	0.05
0.30	0.10	0.05
0.30	0.10	0.10
0.40	0.05	0.20

Initial rate, disappearance of Br₂, Ms^$$-$$1
			5.7$$ \times $$10^$$-$$5
			5.7$$ \times $$10^$$-$$5
			1.2$$ \times $$10^$$-$$4
			3.1$$ \times $$10^$$-$$4

Based on these data, the rate equation is

Rate = k[CH₃COCH₃][Br₂][H⁺]²

Rate = k[CH₃COCH₃][Br₂][H⁺]

Rate = k[CH₃COCH₃][H⁺]

Rate = k[CH₃COCH₃][Br₂]

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