You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Effect of Catalyst

A Chemical re...

Question

A Chemical reaction occurs in three paths having rate constants $k_{1}, k_{2} & k_{3}$ respectively. If $E a_{1}, E a_{2} a n d E a_{3}$ are 4, 5 & 8kJ respectively and overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}} . A s s u m i n g A_{a v} = \frac{A_{1} A_{3}}{A_{2}}$ the overall energy of activation in kJ is ___.

Open in App

Solution

$k_{A V} = A_{(} A V^{.}) e^{- (E_{(} 1) + E_{3} - E_{2}) / R T} ∴ E_{a v} = (4 + 8 - 5) = 7 k J$

Suggest Corrections

Similar questions

Q. A reaction takes place in three steps, the respective rate constants are

k_{1}, k_{2}

and

k_{3}

. The overall rate constant

k = \frac{k_{1} k_{3}}{k_{2}}

. If energies of activation are 40, 30 and 20 kJ, the overall energy of activation is: (assuming 'A' to be constant for all)

Q. A reaction takes place in three steps having rate constants

K_{1}

K_{2}

K_{3}

respectively. The overall rate constant

K = \frac{K_{1} K_{3}}{K_{2}}

. If energies of activation for the three steps 40, 30, 20 kJ respectively, the overall energy of activation is:

Q. A reaction takes place in three steps with an individual rate constant and activation energy, as given below.
Rate constant Activation energy
Step 1

k_{1}

E_{a_{1}} = 180 k J / m o l

Step 2

k_{2}

E_{a_{2}} = 80 k J / m o l

Step 3

k_{3}

E_{a_{3}} = 50 k J / m o l

And overall rate constant,

k = {(\frac{k_{1} k_{2}}{k_{3}})}^{2 / 3}

.
The overall activation energy of the reaction will be:

A reaction takes place in three steps. The rate constant of the three steps are $k_{1}, k_{2}$ and $k_{3}$ respectively. The overall rate constant $k = \frac{k_{1} k_{3}}{k_{2}} .$ The energy of activation for the three steps are 40, 30 and 20 kJ respectively. Therefore:

Q. A reaction takes place in three steps. The rate constant are

k_{1}, k_{2}, a n d k_{3} .

The overall rate constant

k = \frac{k_{1} k_{3}}{k_{2}} .

E_{1}, E_{2} a n d E_{3}

(energy of activation) are 60, 30 and 10 kJ, respectively, the overall energy of activation is:

Join BYJU'S Learning Program

A Chemical reaction occurs in three paths having rate constants k1,k2&k3 respectively. If Ea1,Ea2 and Ea3 are 4, 5 & 8kJ respectively and overall rate constant k=k1k3k2.AssumingAav=A1A3A2 the overall energy of activation in kJ is ___.

kAV=A(AV.)e−(E(1)+E3−E2)/RT∴Eav=(4+8−5)=7kJ

$k_{A V} = A_{(} A V^{.}) e^{- (E_{(} 1) + E_{3} - E_{2}) / R T} ∴ E_{a v} = (4 + 8 - 5) = 7 k J$