For a cell reaction 2H2g-O2g-2H2Ol -rS-298 - -0-32 kJ-K- What is the value of fH-298H2O- l-Given O2g-4H-aq-4e- - 2H2Ol- E- - 1-23 V

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Gibb's Energy and Nernst Equation

For a cell re...

Question

For a cell reaction $2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l); △_{r} S_{298}^{\circ} = - 0.32 k J / K$ . What is the value of $△_{f} H_{298}^{\circ} (H_{2} O, l)$ ?
Given $O_{2} (g) + 4 H^{+} (a q .) + 4 e^{-} ⟶ 2 H_{2} O (l); E^{\circ} = 1.23 V$

- 285.07 k J / m o l

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- 570.14 k J / m o l

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285.07 k J / m o l

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None of these

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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} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 394 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l); Δ H = - 568 k J / m o l

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l); Δ H = - 1058 k J / m o l

C_{(g r a p h i t e s)} + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l);

Δ_{r} H^{\circ} = - 285.8 k J m o l^{- 2}

C O_{2} (g + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g)

Δ_{r} H^{\circ} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{\circ}

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

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