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 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
Given are the values of the rate constants at a certain temperature of some reactions. The fastest reactions is the one with rate constant
k = 3.3 ×10-3 s-1
k = 5.5 × 10-5 s-1
k = 6.6 × 10-6 s-1
k = 4.4 × 10-4 s-1
In the first order reaction
Rate constant is independent of initial concentration
Half life is independent of rate constant
Half lives of liquid state reactions are more than those of gas phase reactions
Half life is independent of activation energy
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
The temperature coefficient of most of the reactions lies between
1 and 3
2 and 3
1 and 4
2 and 4
The sum of powers of the concentration of the reactants in the rate law expression is called
Order of that chemical reaction.
Molecularity of that chemical reaction.
Elementary rate of that chemical reaction.
Average rate of that chemical reaction.
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
The rate at which a substance reacts depends on its
Atomic weight
Equivalent weight
Molecular weight
Active mass
