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
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
The temperature dependance of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k = Ae-E*/RT. Activation energy (E*) of the reaction can be calculated by plotting
log k vs 1/T
k vs T
For the reaction 2N2O5 → 4NO2 + O2, rate and rate constant are 1.02 × 10-4 and 3.4 × 10-5 s -1 respectively, then concentration of N2O5 at that time will be
1.732
3
1.02 × 10-4
3.4 × 105
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 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 a first-order reaction, the half-life period is independent of
Initial concentration
Cube root of initial concentration
First power of final concentration
Square root of final concentration
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
