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In the year 1889, Svante Arrhenius proposed that the dependence of the rate constant ( ) of a…
In the year 1889, Svante Arrhenius proposed that the dependence of the rate constant ($k$) of a reaction on temperature can be expressed by the following equation, known as the Arrhenius equation.
$k = A e^{-E_a/RT}$
The calculation of $E_a$ can be done by using the above equation in the following way:
$\log_{10} k = \log_{10} A - \frac{E_a}{2\cdot303 RT}$
The above equation is similar to the equation for straight line i.e., $y = mx + c$.
It can be used to calculate the value of $E_a$, by using either graphical method or rate constant method.
Read the passage carefully and answer the questions that follow.
(i)[1.0]
The rate of a particular reaction triples when the temperature changes from $30^\circ\text{C}$ to $60^\circ\text{C}$. Calculate the activation energy ($E_a$) of the reaction.
(ii)[1.0]
The slope of the line in the graph of $\log_{10} k$ versus $\frac{1}{T}$ for a reaction is $-4621$. Calculate the energy of activation for the reaction.
(Given: $R = 8\cdot314\text{ J K}^{-1}\text{ mol}^{-1}$)
(iii)[1.0]
What is the order of reaction whose rate constant ($k$) has the same unit as the rate of reaction?
Answer
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From ISC 2025 Improvement Chemistry Paper 1, question 1(C).