The rate constant ( k ) of a reaction is measured at different temperatures (T), and the data are plotted in the given figure. The activation energy of the reaction in kJ mol -1 is: (R is gas constant)

Question

The rate constant ( k ) of a reaction is measured at different temperatures (T), and the data are plotted in the given figure. The activation energy of the reaction in kJ mol -1 is: (R is gas constant) (A) 2R (B) R (C) 1/R (D) 2/R

Tardigrade Admin · Accepted Answer

Slope =-(Ea/R) -(10/5)=-(Ea/R) Ea=2 R

Q. The rate constant $(k)$ of a reaction is measured at different temperatures (T), and the data are plotted in the given figure. The activation energy of the reaction in $k J m o l^{- 1}$ is : (R is gas constant)

2R

R

1/R

2/R

Slope $= - \frac{E _{a}}{R}$

$- \frac{10}{5} = - \frac{E _{a}}{R}$

$E_{a} = 2 R$

Q. The rate constant (k) of a reaction is measured at different temperatures (T), and the data are plotted in the given figure. The activation energy of the reaction in kJmol−1 is : (R is gas constant)

2R

R

1/R

2/R

Slope =−REa​​ −510​=−REa​​ Ea​=2R

Q. The rate constant $(k)$ of a reaction is measured at different temperatures (T), and the data are plotted in the given figure. The activation energy of the reaction in $k J m o l^{- 1}$ is : (R is gas constant)

Slope $= - \frac{E _{a}}{R}$

$- \frac{10}{5} = - \frac{E _{a}}{R}$

$E_{a} = 2 R$