A reaction takes place in various steps- The rate constant for first- second- third and fifth steps are k 1- k 2- k 3 and k 5 respectively- The overall rate constantis given by-k - k 2- k 3- k 1- k 50-5If the activation energies are 40-60-50 and 10 kJ - mol respectively- the overall activation energy kJ - mol is-A- 10B- 20C- None of the aboveD- 25

The correct option is D 25We know that nbsp;Arrhenius equation: k=Ae^ E_a/RT Since we know that rate constant is given as: k=k_2×k_1^0.5k_3 ×k_5^0.5 activati ...

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Standard XII

Chemistry

Arrhenius Equation

A reaction ta...

Question

A reactiontakes place in various steps. The rate constant for first, second, third and fifth steps are $k_{1}, k_{2}, k_{3}$ and $k_{5}$ respectively. The overall rate constant is given by: $k = \frac{k_{2}}{k_{3}} \times (\frac{k_{1}}{k_{5}})^{0.5}$
If the activation energies are 40, 60, 50 and 10 kJ/mol respectively, the overall activation energy (kJ/mol) is:

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None of the above

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Solution

The correct option is C 25
We know that Arrhenius equation:
$k = A e^{- \frac{E_{a}}{R T}}$
Since we know that rate constant is given as:
$k = \frac{k_{2} \times {k_{1}}^{0.5}}{k_{3} \times {k_{5}}^{0.5}}$
activation energy can be given by:
$E_{a} = (E_{2} + 0.5 \times E_{1}) - (E_{3} + 0.5 \times E_{5})$
$E_{a} = 25$

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The correct option is C 25We know that Arrhenius equation: k=Ae−EaRT Since we know that rate constant is given as: k=k2×k10.5k3×k50.5 activation energy can be given by: Ea=(E2+0.5×E1)−(E3+0.5×E5) Ea=25