If 60% of a first order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately
(log 4 = 0.60, log 5 = 0.69)
50 min
45 min
60 min
40 min
Activation energy of a chemical reaction can be determined by
Evaluating rate constant at standard temperature
Evaluating velocities of reaction at two different temperatures
Evaluating rate constants at two different temperatures
Changing concentration of reactants
A substance 'A' decomposes by a first order reaction starting initially with [A] = 2.00m and after 200 min, [A] becomes 0.15 m. For this reaction t1/2 is
53.50 min
50.4 min
48.45 min
46.45 min
A chemical reaction is catalysed by a catalyst X. Hence, X
Reduces enthalpy of the reaction
Decreases rate constant of the reaction
Increases activation energy of the reaction
Does not affect equilibrium constant of the reaction
The rate of first order reaction is 1.5 × 10-2 mol L-1 min-1 at 0.5 M concentration of the reactant. The half-life of the reaction is
0.383 min
23.1 min
8.73 min
7.53 min
For exothermic reaction, the energy of activation of the reactants is
Equal to the energy of activation of products
Less than the energy of activation of products.
Greater than the energy of activation of products.
Sometimes greater and sometimes less than that of the products.
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
For a first order reaction A → B, the reaction rate at reactant concentration of 0.01 M is found to be 2.0 × 10-5 mol L-1s-1. The half-life period of the reaction is
220 s
30 s
300 s
347 s
In a first order reaction A → B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half-life is
