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

The correct option is B 5 kJ mol^ 1 H_2O+O ⇌ nbsp;[E_b]E_a2 HO^∘ Δ H=72kJ T=500 K E_a=77 kJ/mole⇒ nbsp; Δ H=E_a E_b 72=77 E_ ...

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Standard XII

Chemistry

Activation Energy

In gaseous re...

Question

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

5 k J m o l^{- 1}

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149 k J m o l^{- 1}

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10 k J m o l^{- 1}

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None of these

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Solution

The correct option is B $5 k J m o l^{- 1}$
$H_{2} O + O ⇌ [E_{b}] E_{a} 2 H O^{\circ} Δ H = 72 k J$
$T = 500 K$
$E_{a} = 77 k J / m o l e \Rightarrow$ $Δ H = E_{a} - E_{b}$
$72 = 77 - E_{b}$
$E_{b} = 77 - 72$
$E_{b} = 5 k J$

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In gaseous reactions important for understanding the upper atmosphere, H2O and O react biomolecularly to form two OH radicals. ΔH for this reaction is 72 kJ at 500 K and Ea=77kJmol−1, then calculate Ea for the biomolecular recombination of 2OH radicals to form H2O & O at 500 K.

The correct option is B 5kJmol−1H2O+O⇌[Eb]Ea2HO∘ΔH=72kJT=500KEa=77kJ/mole⇒ ΔH=Ea−Eb72=77−EbEb=77−72Eb=5kJ

The correct option is B $5 k J m o l^{- 1}$
$H_{2} O + O ⇌ [E_{b}] E_{a} 2 H O^{\circ} Δ H = 72 k J$
$T = 500 K$
$E_{a} = 77 k J / m o l e \Rightarrow$ $Δ H = E_{a} - E_{b}$
$72 = 77 - E_{b}$
$E_{b} = 77 - 72$
$E_{b} = 5 k J$