Question

Which of the following is correct according to Arrhenius Theory?
where,
$k$ : Rate constant
$E_a$ : Activation energy (in J/mol)
$R$ : Gas constant
$T$ : Temperature of reaction (in Kelvin(K))
$A$ : Arrhenius factor or frequency factor or pre-exponential factor

• A. $k=A{e}^{-E_{a}RT}$
• B. $k=A{e}^{-\frac{E_a}{RT}}$
• C. $k=A{e}^{-\frac{RT}{E_a}}$
• D. $k=A{e}^{-\frac{1}{E_{a}RT}}$

Answer 1

The correct option is B $k=A{e}^{-\frac{E_a}{RT}}$

The method of temperature coefficient was not exact and accurate to explain the effect oftemperature on reaction rate, a new theory was evolved
New thoery:
The temperature dependence of the rate of a chemical reaction can be accurately explained by Arrhenius Theory.
Arrhenius Theory:
For a reaction, relationship between temperature and rate constant follows the equation,
$k=A{e}^{-\frac{E_a}{RT}}$
where,
$k$ : Rate constant
$E_a$ : Activation energy (in J/mol)
$R$ : Gas constant
$T$ : Temperature of reaction (in Kelvin(K))
$A$ : Arrhenius factor or frequency factor or pre-exponential factor. It is constant, specific to a particular reaction