Consider the given plots for a reaction obeying Arrhenius equation `(0^(@)CltTlt300^(@)C)` : (k and `E_(a)` are rate constant and activation energy, respectively)

Consider the given plots for a reaction obeying Arrhenius equation (0^(@)C lt T lt 300^(@)C) : (k and E_(a) are rate constant and activation energy, respectively) Choose the correct option :

Consider the given plots for a reaction obeying Arrhenius equation (k and E_a are rate constant and activation energy, respectively) Choose the correct option:

In Arrhenius equation , k=Ae^(E_a/(RT)) , A may be termed as rate constant .

Rate of a reaction can be expressed by Arrhenius equation as: k = Ae^(-E_(a)//RT) In this equation, E_(a) represents:

In the Arrhenius equation, k = A exp^(-Ea//RT) , A may be termed as the rate constant at…………. .

The Arrhenius equation expressing the effect of temperature on the rate constant of a reaction is given as

For a first order reaction A rarr P , the temperature (T) dependent rate constant (k) was found to follow the equation log k = -2000(1//T) + 6.0 . The pre-exponential factor A and the activation energy E_(a) , respective, are

The variation of rate constant with temperature is given by the integrated from of the Arrhenius equation, log_10k = (-Ea)/(2.303 RT) + constant where k = rate cosntant and Ea is the experimental activation energy. If for a certain reaction, log_10k = (-3163.0)/T + 11.899 , calculate Ea.

A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be k_(1) and k_(2) respectively. Then

State and explain Arrhenius equation. How can we determine the activation energy of a reaction using this equation?