For hydrogen-oxygen fuel cell- the cell reaction is- 2 H 2 g- O 2 g- 2 H 2 OlIf - G f o H 2 O-237-2 kJ mol -1- then emf of this cell is-

The correct option is A +1.23V Gibbs free energy, Δ G ^ o = nF E ^ o ∴ E ^ o =Δ G ^ o nF #160; #160; #160; #160; #160; #160; ...

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Equilibrium Constant from Nernst Equation

For hydrogen-...

Question

For hydrogen-oxygen fuel cell, the cell reaction is:

$2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l)$

If $Δ G_{f}^{o} (H_{2} O) = - 237.2 k J {m o l}^{- 1}$ , then emf of this cell is:

+ 2.46 V

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- 2.46 V

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+ 1.23 V

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- 1.23 V

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Solution

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Similar questions

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l) △ S_{298}^{0} = - 0.32 {kJK}^{- 1}

△_{f} H_{298}^{0} (H_{2} 0, l)

O_{2} (g) + 4 H^{+} (a q) + 4 e^{-} \to 2 H_{2} 0 (l); E^{0} = 1.23 V

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l); △_{r} S_{298}^{\circ} = - 0.32 k J / K

△_{f} H_{298}^{\circ} (H_{2} O, l)

O_{2} (g) + 4 H^{+} (a q .) + 4 e^{-} ⟶ 2 H_{2} O (l); E^{\circ} = 1.23 V

Δ S^{⊖}

2 H_{2} + O_{2} \to 2 H_{2} O

E_{c e l l}^{⊖} = 1.23 V

Δ_{f} H^{⊖} (H_{2} O) = - 285.8 K j m o l^{- 1}

N_{2} H_{4 (a q)} + O_{2 (g)} \to N_{2 (g)} + 2 H_{2} O_{(l)}

Δ G^{0}

E^{0}

H_{2} (g)

O_{2} (g)

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

273 K

9650 sec

C u^{2 +}

1 L

2 M C u S O_{4} (aq)

241.25 sec

P t

p H

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