According to the collision theory of chemical reactions ____.
A chemical reaction occurs with every molecular collision
Rate is directly proportional to the number of collisions per second
Reactions in the gas phase are always of zero order
Reaction rates are of the order of molecular speeds
Activation energy is ____.
The amount of energy to be added to the actual energy of a molecule so that the threshold energy is reached
The amount of energy the molecule must contain so that it reacts
The energy which a molecule should have in order to enter into an effective collision
The average kinetic energy of the molecule
The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by 10oC is ____.
The value of threshold energy increases
Collision frequency increases
The fraction of the molecule having energy equal to threshold energy or more increases
Activation energy decreases
Activation energy of any reaction depends on ____.
Temperature
Nature of reactants
Number of collisions per unit time
Concentration of reactants
Which of the following plots is in accordance with the Arrhenius equation?
Collision theory is applicable to ____.
First order reactions
Zero order reactions
Bimolecular reactions
Intra molecular reactions
A graph plotted between log K vs 1/T for calculating activation energy is shown by ____.
/
k is equilibrium constant
A is adsorption factor
R is Rydberg’s constant
The activation energy of a reaction is zero. The rate constant of this reaction ____.
Increases with increase of temperature
Decreases with an increase of temperature
Decreases with decrease of temperature
Is independent of temperature
An endothermic reaction with high activation energy for the forward reaction is given by the diagram: ____.