H2g - 1 - 2 O2g- 2H2Ol- - H - -86 kJ 2H2g - O2g- 2H2Ol- kJ-

The correct option is A 2H_2(g) + O_2(g)⟶ 2H_2O(l) + 172 kJ .Reaction: H_2(g) + 1 / 2 O_2(g)⟶ 2H_2O(l); nbsp; Δ H = 86 nbsp;kJ ............... ...

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Third Law of Thermodynamics

H2g + 1 / 2 O...

Question

$H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 86 k J$
$2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)$

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) + 172 k J

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2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) - 172 k J

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2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) + 0 k J

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None of these

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H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 286 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)

C_{(s)} + O_{2 (g)} \to C O_{2 (g)};

Δ H = - 394 k J

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

Δ H = - 568 k J

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

Δ H = - 394 k J

C H_{4}

C (s) + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J

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

Δ_{r} H^{\circ} = - 571.8 k J

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

Δ_{r} H^{\circ} = - 890.3 k J

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

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

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

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

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

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