A reaction takes place in three steps- the respective rate constants are k1- k2 and k3- The overall rate constant k - k1 k3-k2- If energies of activation are 40- 30 and 20 kJ- the overall energy of activation is- assuming -A- to be constant for all

The correct option is B 30 K = K_1 K_3/K_2 ∴ ln K = ln #160;K_1 + ln #160;K_3 #160; ln #160;K_2 But #160; ln K = E/RT + ln A ...

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Byju's Answer

Standard XII

Chemistry

Arrhenius Equation

A reaction ta...

Question

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)

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Solution

The correct option is B 30
$K = \frac{K_{1} K_{3}}{K_{2}}$
$∴ l n K = l n K_{1} + l n K_{3} - l n K_{2}$
But $l n K = - \frac{E}{R T} + l n A$
$∴ - \frac{E}{R T} + l n A = - \frac{E_{1}}{R T} + l n A - \frac{E_{3}}{R T} + l n A + \frac{E_{2}}{R T} - l n A$
or, $E_{t o t a l} = E_{1} + E_{3} - E_{2} = 40 + 20 - 30 = 30 k J$

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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: