A reaction takes place in three steps with the rate constant k1- k2 and k3- The overall rate constant k-k1k21-2k3- If activation energies are 40- 30 and 20 kJ for step I- II and III respectively- the overall activation energy of reaction will be-

The correct option is D 35Over all activation energy =E_1+E_22 E_3 =40+302 20 =35 KJ ...

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Standard XII

Chemistry

Activation Energy

A reaction ta...

Question

A reaction takes place in three steps with the rate constant $k_{1}, k_{2}$ and $k_{3}$ . The overall rate constant $k = \frac{k_{1} (k_{2})^{1 / 2}}{k_{3}}$ . If activation energies are $40, 30$ and $20 k J$ for step $I, I I$ and $I I I$ respectively, the overall activation energy of reaction will be:

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Solution

The correct option is D 35
Over all activation energy

$= E_{1} + \frac{E_{2}}{2} - E_{3}$

$= 40 + \frac{30}{2} - 20$

$= 35 K J$

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A reaction takes place in three steps with the rate constant k1,k2 and k3. The overall rate constant k=k1(k2)1/2k3. If activation energies are 40,30 and 20 kJ for step I,II and III respectively, the overall activation energy of reaction will be:

The correct option is D 35Over all activation energy=E1+E22−E3=40+302−20=35KJ

The correct option is D 35
Over all activation energy

$= E_{1} + \frac{E_{2}}{2} - E_{3}$

$= 40 + \frac{30}{2} - 20$

$= 35 K J$