1
AIPMT 2012 Prelims
+4
-1
In a reaction, A + B $$\to$$ product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentration of both the reactants (A and B) are doubled, rate law for the reaction can be written as
A
rate = k[A][B]2
B
rate = k[A]2[B]2
C
rate = k[A][B]
D
rate = k[A]2[B]
2
AIPMT 2012 Prelims
+4
-1
In a zero-order reaction, for every 10oC rise of temperature, the rate is doubled. If the temperature is increased from 10oC to 100oC, the rate of the reaction will become
A
256 times
B
512 times
C
64 times
D
128 times
3
AIPMT 2011 Mains
+4
-1
The rate of the reaction :   2N2O5 $$\to$$ 4NO2 + O2
can be written in three ways.

$${{ - d\left[ {{N_2}{O_5}} \right]} \over {dt}} = k\left[ {{N_2}{O_5}} \right]$$

$${{d\left[ {N{O_2}} \right]} \over {dt}} = k'\left[ {{N_2}{O_5}} \right];\,\,$$ $${{d\left[ {{O_2}} \right]} \over {dt}} = k''\left[ {{N_2}{O_5}} \right]$$

The relationship between k and k' and between k and k'' are
A
$$k' = 2k ; k'' = k$$
B
$$k' = 2k ; k'' = k/2$$
C
$$k' = 2k ; k'' = 2k$$
D
$$k' = k ; k'' = k$$
4
AIPMT 2011 Mains
+4
-1
The unit of rate constant for a zero order reaction is
A
mol L$$-$$1 s$$-$$1
B
L mol$$-$$1 s$$-$$1
C
L2 mol$$-$$2 s$$-$$1
D
s$$-$$1
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