For a cell reaction
2H₂(g) + O₂(g) → 2H₂O(l)
ΔS°₂₉₈ = –0.32 kJ/K
What is the value of Δ_fH°(298) (H₂O, l)?

[Given: standard electrode potential of the following half cell reaction is 1.23 V, O₂(g) + 4H⁺ + 4e^– → 2H₂O(l)]

दी गयी सेल अभिक्रिया
2H₂(g) + O₂(g) → 2H₂O(l) के लिए
ΔS°₂₉₈ = –0.32 kJ/K
Δ_fH°(298) (H₂O, l) का मान क्या है?

[दिया गया है : अर्ध सेल अभिक्रिया O₂(g) + 4H⁺ + 4e^– → 2H₂O(l) का मानक इलेक्ट्रॉड विभव 1.23 V है]

–285.07 kJ/mol

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–28.507 kJ/mol

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–570.17 kJ/mol

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570.14 kJ/mol

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Solution

The correct option is A –285.07 kJ/mol
Solution

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Similar questions

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

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

O_{2} (g)

⎡ ⎢ ⎢ ⎢ ⎢ ⎢ ⎣ \begin{matrix} (c o r r e c t) C u (s) ⟶ & C u^{2 +} (a q) + 2 e^{-} E_{C u | C u^{2 +}}^{⊝} = - 0.34 V (w r o n g) 2 H_{2} O (l) ⟶ & O_{2} (g) + 4 H^{\oplus} (a q) + 4 e^{-} E_{H_{2} O | O_{2}}^{⊝} = - 1.23 V \end{matrix} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦

\begin{matrix} I n (d) \end{matrix}

⎡ ⎢ ⎢ ⎢ ⎢ ⎢ ⎢ ⎢ ⎢ ⎣ \begin{matrix} (c o r r e c t) N i (s) ⟶ & N i^{2 +} (a q) + 2 e^{-} E_{N i | N i^{2 +}}^{⊝} = - 0.25 V (w r o n g) 4 ⊝ O H (a q) ⟶ & O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} E_{⊝ O H | O_{2}}^{\oplus} = - 0.4 V \end{matrix} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦

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

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