Consider the following plots of rate constant versus (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 constant versus (1/T) for four different reactions. which of the following orders is correct for the activation energies of these reactions? <img class="img-fluid question-image" alt="Question" src="https://cdn.tardigrade.in/q/nta/c-wryv1ldbhcvpstjl.jpg" /> (A) Ec>Ea>Ed>Eb (B) Eb>Ea>Ed>Ec (C) Ea>Ec>Ed>Eb (D) Eb>Ed>Ec>Ea

Tardigrade Admin · Accepted Answer

As we know that Arrhenius equation is given as K= textA texte- (Ea/ textRT) log K=log â¡ A-(Ea/2.303 R T) textSlope=-(Ea/2.303 text R) Slope c>a>d>b. Ec>Ea>Ed>Eb

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

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

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

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

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

As we know that Arrhenius equation is given as
$K = A e^{- \frac{E _{a}}{RT}}$
$l o g K = l o g A - \frac{E _{a}}{2.303 RT}$
$Slope = - \frac{E _{a}}{2.303 R}$
Slope $c > a > d > b .$
$E_{c} > E_{a} > E_{d} > E_{b}$

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

Ec​>Ea​>Ed​>Eb​

Eb​>Ea​>Ed​>Ec​

Ea​>Ec​>Ed​>Eb​

Eb​>Ed​>Ec​>Ea​