In the reaction,
BrO$$_{3(aq)}^ - $$ + 5Br$$_{(aq)}^ - $$ + 6H+ $$ \to $$ 3Br2(l) + 3H2O(l).
The rate of appearance of bromine (Br2) is related to rate of disappearance of bromide ions as
For the reaction, N2 + 3H2 $$ \to $$ 2NH3, if
$${{d\left[ {N{H_3}} \right]} \over {dt}}$$ = 2 $$ \times $$ 10$$-$$4 mol L$$-$$1 s$$-$$1,
the value of $${{ - d\left[ {{H_2}} \right]} \over {dt}}$$ would be
The bromination of acetone that occurs in acid solution is represented by this equation.
CH3COCH3(aq) + Br2(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
A
Rate = k[CH3COCH3][Br2][H+]2
B
Rate = k[CH3COCH3][Br2][H+]
C
Rate = k[CH3COCH3][H+]
D
Rate = k[CH3COCH3][Br2]
Explanation
From the first two experiments, it is clear
that when concentration of Br2
is doubled, the initial
rate of disappearance of Br2
remains unaltered. So,
order of reaction with respect to Br2
is zero. The
probable rate law for the reaction will be :
k[CH3COCH3
][H+].
4
AIPMT 2008
MCQ (Single Correct Answer)
The rate constants k1 and k2 for two different reactions are 1016 $$ \cdot $$ e$$-$$2000/T and 1015 $$ \cdot $$ e$$-$$1000/T, respectively.
The temperature at which k1 = k2 is