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

H_2O+O⟶ 2OH; Δ H=72 KJ at 500 K; Given E_a=77 nbsp;KJmol^ 1 2OH⟶ H_2O+O; E_a_3.2 For a reaction E_a =Δ H+E_a_3.2 ∴ 77=72+E_a_3.2 ∴ nbsp;E_a_3.2=5 KJmol^ 1 ...

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Standard XII

Chemistry

Activation Energy

In gaseous re...

Question

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:

$3$ kJ mol^-1

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$4$ kJ mol^-1

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$5$ kJ mol^-1

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$7$ kJ mol^-1

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Solution

The correct option is C
$5$ kJ mol^-1

$H_{2} O + O ⟶ 2 O H; Δ H = 72 KJ at 500 K;$
Given $E_{a} = 77 {KJmol}^{- 1}$
$2 O H ⟶ H_{2} O + O; E_{a_{3.2}}$
For a reaction $E_{a} = Δ H + E_{a_{3.2}}$
$∴ 77 = 72 + E_{a_{3.2}}$
$∴ E_{a_{3.2}} = 5 {KJmol}^{- 1}$

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In gaseous reactions important for the understanding of the upper atmosphere H2O and O react bimolecularly to form two OH radicals. ΔH for this reaction is 72 kJ at 500 K and Ea is 77 kJ mol-1, then Ea for the bimolecular recombination of two OH radicals to form H2O and O is:

The correct option is C 5 kJ mol-1 H2O+O⟶2OH;ΔH=72 KJ at 500 K; Given Ea=77 KJmol−1 2OH⟶H2O+O; Ea3.2 For a reaction Ea=ΔH+Ea3.2 ∴77=72+Ea3.2 ∴Ea3.2=5 KJmol−1

The correct option is C
$5$ kJ mol^-1

$H_{2} O + O ⟶ 2 O H; Δ H = 72 KJ at 500 K;$
Given $E_{a} = 77 {KJmol}^{- 1}$
$2 O H ⟶ H_{2} O + O; E_{a_{3.2}}$
For a reaction $E_{a} = Δ H + E_{a_{3.2}}$
$∴ 77 = 72 + E_{a_{3.2}}$
$∴ E_{a_{3.2}} = 5 {KJmol}^{- 1}$