For a reaction between A and B the order with respect to A is 2 and the other with respect to B is 3. The concentrations of both A and B are doubled, the rate will increase by a factor of
A
12
B
16
C
32
D
10
Explanation
Rate1 = k[A]2[B]3
when concentrations of both A and B are
doubled then
Rate2 = k[2A]2[2B]3 = 32 k[A]2[B]3
$$ \therefore $$ Rate will increase by a factor of 32.
4
AIPMT 2012 Prelims
MCQ (Single Correct Answer)
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
Explanation
For energy 10° rise in temperature the rate of
reaction doubles. So, rate = 2n when, n = 1 rate = 21
= 2
when, temperature is increased from 10°C to 100°C
change in temperature = 100 – 10 = 90°C
i.e., n = 9
So, rate = 29
= 512 times
Questions Asked from Chemical Kinetics
On those following papers in MCQ (Single Correct Answer)
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