A large increase in the rate of a reaction for a rise in temperature is due to ____.
The decrease in the number of collisions
The increase in the number of activated molecules
The shortening of the mean free path
The lowering of the activation energy
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
According to the collision theory of reaction rates, rate of reaction increases with temperature due to ____.
Greater number of collisions
Greater velocity of the reacting molecules
Greater number of molecules have activation energy
None of the above
The reaction rate at a given temperature becomes slower, then ____.
The free energy of activation is higher
The free energy of activation is lower
The entropy changes
The initial concentration of the reactants remains constant
The minimum energy a molecule should possess in order to enter into a fruitful collision is known as ____.
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
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
An endothermic reaction with high activation energy for the forward reaction is given by the diagram: ____.