1
AIPMT 2009
MCQ (Single Correct Answer)
+4
-1
Half-life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is
A
0.5 $$ \times $$ 10$$-$$2 s$$-$$1
B
0.5 $$ \times $$ 10$$-$$3 s$$-$$1
C
5.0 $$ \times $$ 10$$-$$2 s$$-$$1
D
5.0 $$ \times $$ 10$$-$$3 s$$-$$1.
2
AIPMT 2008
MCQ (Single Correct Answer)
+4
-1
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]
3
AIPMT 2008
MCQ (Single Correct Answer)
+4
-1
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
A
2000 K
B
$${{1000} \over {2.303}}K$$
C
1000 K
D
$${{2000} \over {2.303}}K$$
4
AIPMT 2007
MCQ (Single Correct Answer)
+4
-1
The reaction of hydrogen and iodine monochloride is given as :
H2(g) + 2ICl(g) $$ \to $$ 2HCl(g) + I2(g)
This reaction is of first order with respect to H2(g) and ICl(g),
following mechanisms were proposed.

Mechanism A :
     H2(g) + 2ICl(g) $$ \to $$ 2HCl(g) + I2(g)
Mechanism B :
     H2(g) + ICl(g) $$ \to $$ HCl(g) + HI(g) ; slow
     HI(g) + ICl(g) $$ \to $$ HCl(g) + I2(g) ; fast

Which of the above mechanism(s) can be consistent with the given information about the reaction?
A
A and B both
B
Neither A nor B
C
A only
D
B only
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