Consider two reactions, A and B. Reaction A has a higher activation energy than reaction B. Which statement is most likely true?
Reaction A will proceed faster than reaction B at the same temperature.
Both reactions will proceed at the same rate at the same temperature.
Reaction B will proceed faster than reaction A at the same temperature.
The relative rates of reactions A and B cannot be predicted based on activation energy alone.
Related Questions
A reaction between gases X and Y follows the rate law: Rate = k[X]Β²[Y]. If the concentration of X is tripled and the concentration of Y is halved, the new rate will be:
1.5 times the original rate
4.5 times the original rate
9 times the original rate
0.75 times the original rate
The minimum energy required for a reaction to occur is called:
Kinetic energy
Potential energy
Activation energy
Ionization energy
For producing the effective collision, the colliding molecules must possess
A certain minimum amount of energy
Energy equal or greater than threshold energy
Proper orientation
Threshold energy as well as proper orientation
The minimum energy a molecule should posses in order to enter into a fruitful collision is known as
Reaction energy
Collision energy
Activation energy
Threshold energy
For producing the effective collisions the colliding molecules must have:
A certain minimum amount of energy
Energy lesser than threshold energy
Improper orientation
Proper orientation and energy equal or greater than threshold energy
For a reaction to occur according to collision theory, the colliding molecules must have:
Energy less than the activation energy and proper orientation
Energy greater than or equal to the activation energy and any orientation
Energy less than the activation energy and any orientation
Energy greater than or equal to the activation energy and proper orientation
The pre-exponential factor (A) in the Arrhenius equation is related to the:
Activation energy of the reaction
Enthalpy change of the reaction
Frequency of collisions with proper orientation
Temperature of the reaction
According to collision theory, for a reaction to occur, colliding molecules must have:
Sufficient energy
Proper orientation
Sufficient energy and proper orientation
Low energy and any orientation
Increasing the temperature generally increases the reaction rate because:
The activation energy decreases
More molecules have sufficient energy to react
The concentration of reactants increases
The molecules become larger
According to collision theory:
Collisions are sufficiently violent
All collision are responsible for reaction
All collisions are effective
Only highly energetic molecules have enough energy to react
