The units of rate of a reaction and rate constant are identical for a
Zero order reaction
Fractional order reaction
First order reaction
Second order reaction
The experimental rate law for the reaction, A + 2B → C is r = k[A][B]2 If the concentration of both A and B are doubled, the rate of the reaction increases by a factor of
2
4
4√2
2√2
The temperature coefficient of most of the reactions lies between
1 and 3
2 and 3
1 and 4
2 and 4
For the reaction CO + Cl2 → COCl2, the rate is given by, r = k [COCl2]3/2. The unit of the reaction rate is
L-1
s-1
mol3/2 L-3/2 s-1
L-1 mol s-1
The rate constants k1 and k2 for two different reaction are 1016.e-2000/T and 1015.e-1000/T, respectively. The temperature at which k1 = k2 is
1000 K
2000 K
The temperature dependence of the rate constant is given by the Arrhenius equation as
ln k = ln A - Ea/RT
ln A = ln k - Ea/RT
ln k = A Ea/RT
ln A = RT ln Ea - ln k
The half life period of a first order reaction
Increases with increasing temperature
Increases with decreasing temperature
Is not affected by changing temperature
Increases firstly followed by a decrease on increasing temperature
The reaction 2FeCl3 + SnCl2 → 2FeCl2 + SnCl4 is an example of
Third order reaction
None of these
For the reaction
2 A + B → 3C + D
Which of the following does not express the reaction rate?
The rate of a reaction is doubled for every 100 rise in temperature. The increase in reaction rate as a result of temperature rise from 100 to 1000 is how much times?
112
512
400
614
