A reaction takes place in various steps. The rate constants for the first, second, third and fifth steps are \(k_1,k_2,k_3\) and \(k_5,\) respectively. The overall rate constant is given by \[k=\dfrac{k_2}{k_3}\left (\dfrac{k_1}{k_5}\right )^{0.5}.\]
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If the activation energies are 40, 60, 50 and 10 kJ/mol, respectively, what is the overall energy of activation (in kJ/mol)?

**Note:** The above image is not the described reaction.

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