Answer
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Hint: The pre-exponential factor or A factor is the pre-exponential constant in the Arrhenius equation, an empirical relationship between temperature and rate coefficient. It is usually designated by A when determined from experiment, while Z is usually left for collision frequency.
Complete answer:
The Arrhenius equation gives the dependence of the rate constant of a chemical reaction on the absolute temperature as:
\[k=A{{e}^{-\dfrac{E_a}{RT}}}\]
where
k is the rate constant (frequency of collisions resulting in a reaction),
T is the absolute temperature (in kelvins),
A is the pre-exponential factor, a constant for each chemical reaction,
$E_a$ is the activation energy for the reaction (in the same units as RT),
R is the universal gas constant.
A first-order reaction is a reaction that proceeds at a rate that depends linearly on only one reactant concentration.
Taking the natural logarithm of Arrhenius equation yields:
\[\ln k=\ln A-\dfrac{E_a}{RT}\]
Putting the values as given in the question we get,
\[\begin{align}
& {{\log }_{e}}k={{\log }_{e}}A-\dfrac{E_a}{RT} \\
& \Rightarrow {{\log }_{10}}k={{\log }_{10}}A-\dfrac{E_a}{2.303RT} \\
&\Rightarrow {{\log }_{10}}A=6 \\
&\Rightarrow A={{10}^{6}} \\
\end{align}\]
Also, activation energy will be,
\[\begin{align}
& \Rightarrow \dfrac{E_a}{R\times 2.303}=2000 \\
& \Rightarrow E_a=38.3\times {{10}^{3}}J/mol \\
& \Rightarrow E_a=38.3kJ/mol \\
\end{align}\]
Therefore, the correct answer is the D option.
Note:
Activation energy is the energy that must be provided to compounds to result in a chemical reaction. The activation energy ($E_a$) of a reaction is measured in joules per mole (J/mol), kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).
Complete answer:
The Arrhenius equation gives the dependence of the rate constant of a chemical reaction on the absolute temperature as:
\[k=A{{e}^{-\dfrac{E_a}{RT}}}\]
where
k is the rate constant (frequency of collisions resulting in a reaction),
T is the absolute temperature (in kelvins),
A is the pre-exponential factor, a constant for each chemical reaction,
$E_a$ is the activation energy for the reaction (in the same units as RT),
R is the universal gas constant.
A first-order reaction is a reaction that proceeds at a rate that depends linearly on only one reactant concentration.
Taking the natural logarithm of Arrhenius equation yields:
\[\ln k=\ln A-\dfrac{E_a}{RT}\]
Putting the values as given in the question we get,
\[\begin{align}
& {{\log }_{e}}k={{\log }_{e}}A-\dfrac{E_a}{RT} \\
& \Rightarrow {{\log }_{10}}k={{\log }_{10}}A-\dfrac{E_a}{2.303RT} \\
&\Rightarrow {{\log }_{10}}A=6 \\
&\Rightarrow A={{10}^{6}} \\
\end{align}\]
Also, activation energy will be,
\[\begin{align}
& \Rightarrow \dfrac{E_a}{R\times 2.303}=2000 \\
& \Rightarrow E_a=38.3\times {{10}^{3}}J/mol \\
& \Rightarrow E_a=38.3kJ/mol \\
\end{align}\]
Therefore, the correct answer is the D option.
Note:
Activation energy is the energy that must be provided to compounds to result in a chemical reaction. The activation energy ($E_a$) of a reaction is measured in joules per mole (J/mol), kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).
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