g Which statement is false? According to the rate law, the greater the rate constant (k), the faster the rate of reaction is. According to the Arrhenius equation, the greater the collision frequency of molecules (A), the greater the rate constant (k) is. According to the Arrhenius equation, the greater the activation energy of the reaction (Ea), the greater the rate constant (k) is. According to the Arrhenius equation, the greater the temperature of reaction (T), the greater the rate constant (k) is.

Rate law in chemistry describes the relationship between the concentration of reactants and the rate of reaction. In the rate law expression i.e. Rate = K {X}, K is the proportionality constant called RATE CONSTANT. The greater the value of this rate constant (k), the faster the rate of reaction is.

According to the Arrhenius equation, mathematically written as:

K= Ae (-EA/RT) where; k is the rate constant, Ea is the activation energy, T= temperature, R= gas constant.

- The collision frequency of molecules is dependent on the temperature, which when increases causes an increase in the rate constant.

- In the presence of a catalyst, the activation energy is lowered causing the rate of reaction to increase, meaning that the rate constant is increased. Hence, the GREATER the activation energy of the reaction (Ea), the LOWER the rate constant (k) is.

- An increase in temperature causes the rate of constant (K) to increase.