- G- for the following reaction is- 4A1 - 3O2 - 6H2O - 4 - OH - 4A1OH4 - E-cell - 2-73 V - fG- OH - -157 kJ mol-1 - fG-H2O - -237 kJ mol-1

The correct option is A 3.16 × 10^3 kJ mol^ 1 As we know, Δ_rG^⊖_cell = n_cellFE^⊖_cell = 12 × 96500 × 2.73 = 3.16 × 10^3 kJ mol ...

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Nernst Equation

Δ G⊖ for the ...

Question

$Δ G^{⊖}$ for the following reaction is:
$4 A 1 + 3 O_{2} + 6 H_{2} O + 4 ⊖ O H \to 4 A 1 (O H)_{4}^{⊖}$
$E_{c e l l}^{⊖} = 2.73 V$
$Δ_{f} G_{(⊖ O H)}^{⊖} = - 157 k J m o l^{- 1}$
$Δ_{f} G_{(H_{2} O)}^{⊖} = - 237 k J m o l^{- 1}$

- 3.16 \times 10^{3} k J m o l^{- 1}

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- 0.79 \times 10^{3} k J m o l^{- 1}

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- 0.263 \times 10^{3} k J m o l^{- 1}

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+ 0.263 \times 10^{3} k J m o l^{- 1}

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Solution

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Similar questions

4 A l (s) + 3 O_{2} (g) + 6 H_{2} O + 4 ⊖ O H \to 4 [A l (O H)_{4}]^{\oplus}

E_{c e l l}^{⊖} = 2.73 V

Δ_{f} G^{⊖} [\oplus O H] = - 157 k J m o l^{- 1}

Δ_{f} G^{⊖} (H_{2} O) = - 237.2 k J m o l^{- 1}

Δ_{f} G^{⊖} [A l (O H)_{4}]^{⊖}

(A l (O H)_{4}^{⊖}]

4 A l (s) + 3 O_{2} (g) + 6 H_{2} O + 4 O H^{-} ⇋ 4 [A l (O H)_{4}^{-}]

E_{c e l l}^{\circ} = 2.73 V

Δ G_{f}^{\circ} (O H^{-}) = 157 k J m o l^{- 1}

Δ G_{f}^{\circ} (H_{2} O) = - 237.2 k j m o l^{- 1}

Δ G_{f}^{\circ} [A l (O H)_{4}]

l o g_{10} (k_{2})

k_{2}

293 K

103 k J m o l^{- 1}

273 K i s 7.87 \times 10^{- 7} s^{- 1}

l o g_{10} (7.87) \approx 0.9

E_{c e l l}^{o}

4 A l (s) + 3 O_{2} (s) + 6 H_{2} O + 4 O H^{-} \to 4 [A l (O H)_{4}^{-}]

△ G_{f}^{o}

O H^{-}

H_{2} O

^{- 1}

^{- 1}

△ G_{f}^{o}

[A l (O H)_{4}]^{-}

x

- x

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