According to arrhenius equation, the slope of log k vs (1/ T ) plot is:

Question

According to arrhenius equation, the slope of log k vs (1/ T ) plot is: (A) (-Ea/2.303 R) (B) (- E a /2.303) (C) (- E a /2.303 RT ) (D) (Ea/2.303 R T)

Tardigrade Admin · Accepted Answer

Arrhenius equation is k = Ae - Ea / RT on taking log on both sides, we get, log k = log A -( E a /2.303 RT ) When log K is plotted with 1 / T, the slope of the reaction will be (- E a /2.303 R ) and intercept given by log A

Q. According to arrhenius equation, the slope of $lo g k$ vs $\frac{1}{T}$ plot is:

$\frac{- E _{a}}{2.303 R}$

$\frac{- E _{a}}{2.303}$

$\frac{- E _{a}}{2.303 RT}$

$\frac{E _{a}}{2.303 RT}$

Arrhenius equation is $k = A e^{- E a / RT}$

on taking log on both sides,

we get, $lo g k = lo g A - \frac{E _{a}}{2.303 RT}$

When $lo g K$ is plotted with $1/ T$ , the slope of the reaction

will be $\frac{- E _{a}}{2.303 R}$ and intercept given by $lo g A$

Q. According to arrhenius equation, the slope of logk vs T1​ plot is:

2.303R−Ea​​

2.303−Ea​​

2.303RT−Ea​​

2.303RTEa​​