Calculate the equilibrium constant for the reaction- Zns - Ag2Os - H2Ol - 2Ags - Zn2-aq- - 2OH-aq-when Ecell- - 1-11 at 298 K-

The correct option is B 4.599× 10^37 . E^∘_cell=RTnFln× K ⟹ 1.11=8.314× 2982× 96500ln× K ⟹ 1.11=0.0128× ln× K ⟹ K=e^86.7188=4.587× 10^37 ...

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Equilibrium Constant from Nernst Equation

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Question

Calculate the equilibrium constant for the reaction,
$Z n (s) + A g_{2} O (s) + H_{2} O (l) \to 2 A g (s) + Z n^{2 +} (a q .) + 2 O H^{-} (a q .)$
when $E_{c e l l}^{\circ} = 1.11$ at $298 K$ .

2.499 \times 10^{37}

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2.499 \times 10^{35}

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3.499 \times 10^{35}

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4.599 \times 10^{37}

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Solution

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△ G^{\circ}

Z n (s) + A g_{2} O (s) + H_{2} O (l) ⇌ Z n^{2 +} (a q) + 2 A g (s) + 2 O H^{-} (a q)

E_{A g^{+} / A g}^{\circ} = + 0.80 V

E_{Z n^{2 +} / Z N}^{\circ} = - 0.76 V

Δ G

Z n_{(s)} + A g_{2} O_{(s)} + H_{2} O_{(l)} \to Z n_{(a q)}^{2 +} + 2 A g_{(s)} + 2 O H^{-}_{(a q)}

E_{{A g}^{+} / A g}^{0} = + 0.80 V

E_{{Z n}^{+ 2} / Z n}^{0} = - 0.76 V

Δ_{r} G^{o}

Z n_{(s)} + A g_{2} O_{(s)} + H_{2} O_{(l)} \to Z n_{(a q)}^{2 +} + 2 A g_{(s)} + 2 O H_{(a q)}^{-}

[E_{A g_{2} O / A g}^{o} = 0.344 V, E_{Z n^{2 +} / Z n}^{o} = - 0.76 V]

Z n (s) + A g_{2} O (s) + H_{2} O (l) ⇌ 2 A g (s) + Z n^{2 +} (a q) + 2 O H^{-} (a q)

Z n^{2 +} (a q) + 2 e^{-} \to Z n (s); E^{\circ} = - 0.76 V

A g_{2} O (s) + H_{2} O (l) + 2 e^{-} \to 2 A g (s) + 2 O H^{-} (a q), E^{\circ} = 0.34 V

Z n (s) + A g_{2} O (s) + H_{2} O (l) ⇌ 2 A g (s) + Z n^{2 +} (a q) + 2 O H^{-} (a q)

Z n^{2 +} (a q) + 2 e \to Z n (s); E^{0} = - 0.76 V

A g_{2} O (s) + H_{2} O (l) 2 e \to 2 A g (s) + 2 O H^{-} (a q), E^{0} = 0.34 V

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