Consider the following plots of rate Consider the following plots of rate (1/T) for four different reactions. Which of the following orders is correct for the activation energies of these reactions ?

Question

Consider the following plots of rate Consider the following plots of rate (1/T) for four different reactions. Which of the following orders is correct for the activation energies of these reactions ? (A) Eb > Ea > Ed > Ec (B) Ea > Ec > Ed > Eb (C) Eb > Ed > Ec > Ea (D) Ec > Ea > Ed > Eb

Tardigrade Admin · Accepted Answer

log K=(-Ea/2.3030RT)+log A Acrroding to Arrhenius equation plot of 'log K' Vs. (1/T) is linear with. Slope =(-Ea/2.3030R) From plot we conclude: underset text(magnitude) text|Slope|: C>a>d>b ∴ Ec>Ea>Ed>Eb

Q. Consider the following plots of rate Consider the following plots of rate $\frac{1}{T}$ for four different reactions. Which of the following orders is correct for the activation energies of these reactions ?

$E_{b} > E_{a} > E_{d} > E_{c}$

$E_{a} > E_{c} > E_{d} > E_{b}$

$E_{b} > E_{d} > E_{c} > E_{a}$

$E_{c} > E_{a} > E_{d} > E_{b}$

$l o g K = \frac{- E a}{2.3030 RT} + l o g A$
Acrroding to Arrhenius equation plot of $^{'} l o g K^{'}$
$V s . \frac{1}{T}$ is linear with.
Slope $= \frac{- E a}{2.3030 R}$
From plot we conclude :
$(magnitude) |Slope| : C > a > d > b$
$∴ E_{c} > E_{a} > E_{d} > E_{b}$

Q. Consider the following plots of rate Consider the following plots of rate T1​ for four different reactions. Which of the following orders is correct for the activation energies of these reactions ?

Eb​>Ea​>Ed​>Ec​

Ea​>Ec​>Ed​>Eb​

Eb​>Ed​>Ec​>Ea​

Ec​>Ea​>Ed​>Eb​