Question

Arrhenius equation is:

• A. $\left(d/dT\right)lnK=-\left(\Delta E/R{T}^2\right)$
• B. $\left(d/dT\right)lnK=+\left(E_a/R{T}^2\right)$
• C. $\left(d/dT\right)lnK=-\left(\Delta E/RT\right)$
• D. $K=A{e}^{-E_a/RT}$

Answer 1

Answer: (B), (D)

The correct options are
B $\left(d/dT\right)lnK=+\left(E_a/R{T}^2\right)$
D $K=A{e}^{-E_a/RT}$

As we know, the higher the temperature, the faster a given chemical reaction will proceed. Quantitatively, this relationship between the rate a reaction proceeds and its temperature is determined by the Arrhenius Equation.

It is given by

$K=A{e}^{(-E_a/RT)}$

On differentiating the above equation we get,

$\left(d/dT\right)lnK=+\left(E_a/R{T}^2\right)$

Therefore rate constant decreases with temperature.
Thus, as temperature increases, the rate constant increases and approaches a value close to the Arrhenius constant.

Therefore option B is also correct answer