Question

if the activation energy required for a chemical reaction were reduced, what would happen to the rate of the reaction? the rate would increase. the rate would decrease. the rate would remain the same. the rate would be zero.

Explanation:

Step1: Recall reaction - rate and activation - energy relationship

The rate of a chemical reaction is related to the activation energy by the Arrhenius equation $k = A e^{-\frac{E_a}{RT}}$, where $k$ is the rate - constant, $A$ is the pre - exponential factor, $E_a$ is the activation energy, $R$ is the gas constant, and $T$ is the temperature. When the activation energy $E_a$ decreases, the exponent $-\frac{E_a}{RT}$ becomes less negative.

Step2: Analyze the effect on the rate - constant

As $-\frac{E_a}{RT}$ becomes less negative, the value of $e^{-\frac{E_a}{RT}}$ increases. Since the rate of the reaction is proportional to the rate - constant $k$, and $k$ increases when $E_a$ decreases, the rate of the reaction increases.

Answer:

The rate would increase.