In gaseous reaction important for the understanding of the upper atmosphere H 2 O and O react bimolecularly to form two OH radicals- - H for this reaction is 72 kJ at 500 K and E a is 77 kJ mol -1 E a for the bimolecular recombination of two OH radicals to form H2O and O is- in kJ mol -1

The reaction is: H_2O+O⟶ 2OH , #160; #160; #160; #160; #160; #160; Δ H= 72 kJ ; E_a=77kJ/mol 2OH⟶ H_2O+O , #160; #160 ...

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Byju's Answer

Standard XII

Chemistry

Activation Energy

In gaseous re...

Question

In gaseous reaction important for the understanding of the upper atmosphere $H_{2} O$ and $O$ react bimolecularly to form two $O H$ radicals. $Δ H$ for this reaction is 72 kJ at 500 K and $E_{a}$ is 77 kJ ${m o l}^{- 1}$ $E_{a}$ for the bimolecular recombination of two OH radicals to form $H_{2} O$ and $O$ is:
(in kJ ${m o l}^{- 1}$ )

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Solution

The reaction is:
$H_{2} O + O ⟶ 2 O H$ , $Δ H = - 72 k J$ ; $E_{a} = 77 k J / m o l$
$2 O H ⟶ H_{2} O + O$ , $E_{a} = ?$ (Refer to Image)
$E_{a}$ for the reverse reaction
$= (E_{a})_{f o r w a r d} + Δ H$
$= 77 + (- 72) = 5 k J$

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In gaseous reactions important for the understanding of the upper atmosphere $H_{2} O$ and $O$ react bimolecularly to form two $O H$ radicals. $Δ H$ for this reaction is $72$ kJ at $500$ K and $E_{a}$ is $77$ kJ mol^-1, then $E_{a}$ for the bimolecular recombination of two $O H$ radicals to form $H_{2} O$ and $O$ is: