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
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
For producing effective collisions the colliding molecules must have
A certain minimum amount of energy
Energy equal to or greater than threshold energy
Proper orientation
Both threshold energy and proper orientation
The correct statement is
The rate constant of an exothermic reaction decreases with increase in temperature
The rate constant of an endothermic reaction increases with increase in temperature
The rate constant of forward and backward directions of a reversible reaction decreases with increase in temperature
The rate constant of forward direction increases while that of backward reaction decreases with increase in temperature.
The rate of reaction between two reactants A and B decreases by a factor of 4, if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is
-1
-2
1
2
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
53.49 min
50.49 min
48.45 min
46.45 min
The reaction 2FeCl3 + SnCl2 → 2FeCl2 + SnCl4 is an example of
First order reaction
Second order reaction
Third order reaction
None of these
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
In the case of a first order reaction, when log k (y-axis) is plotted against 1/T, a straight line graph with slope -1.25×104 is obtained. The energy of activation for the reaction is
28.78 kJ mol-1
2.77 kJ mol-1
239.34 kJ mol-1
27.7 kJ mol-1
