In gaseous reaction important for understanding the upper atmosphere- H2O and O react bimolecularly to form two OH radicals- - H for this reaction is 72 J at 500 K and Ea - 77 kj mol-1- then calculate Ea for the bimolecular recombination of 2OH radicals to form H2O and O at 500 K-

H_2O+O ⟶ 2OH ⇒Δ H= 72 kJ E_α=77 kJ /mole (given) ⇒ 2OH ⟶ H_2O+O ⇒ 77= 72+E_α ⇒ E_α=5kJ/mol ...

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Standard XII

Chemistry

Activation Energy

In gaseous re...

Question

In gaseous reaction important for understanding the upper atmosphere, $H_{2} O$ and $O$ react bimolecularly to form two $O H$ radicals. $Δ H$ for this reaction is $72 J$ at $500 K$ and $E_{a} = 77 k j m o l^{- 1}$ , then calculate $E_{a}$ for the bimolecular recombination of $2 O H$ radicals to form $H_{2} O$ and $O$ at $500 K$ .

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Solution

$H_{2} O + O ⟶ 2 O H \Rightarrow Δ H = 72 k J$
$E_{α} = 77 k J / m o l e$ (given)
$\Rightarrow 2 O H ⟶ H_{2} O + O$
$\Rightarrow 77 = 72 + E_{α}$
$\Rightarrow E_{α} = 5 k J / m o l$

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