Question

The Arrhenius equation describes the relationship between the rate constant and the energy of activation

where k is the rate constant of the reaction. A is the frequency factor, E, is the activation energy, R is the ideal gas constat, and T' is the absolute temperature.
Based on the Arrhenius equation, which of the statements is true?
a.Al curstant energy of activation, reactions at lower temperatures proceed more rapidly
b.At constant temperature, reactions with lower activation energies procced less rapidly.
c.Al constant femperieure, reactions with lower activation energies proceed more rapidly.
d.Atene fårt erergy of activation, reactions with smaller values of A proceed more rapidly

Answer 1

At constant temperature, reactions with lower activation energies proceed more rapidly, as the lower energy barrier allows for more successful molecular collisions.

Step-by-step explanation:

The Arrhenius equation (k = Ae-Ea/RT) describes the relationship between the rate constant (k), activation energy (Ea), frequency factor (A), ideal gas constant (R), and absolute temperature (T). This equation tells us how various factors affect the rate at which reactions proceed. Among the given statements, the true one is that at constant temperature, reactions with lower activation energies proceed more rapidly. This is because a lower activation energy means there is a lower energy barrier for the reaction to occur, allowing more molecular collisions to result in successful reactions.