2 H 2 g - O 2 g - 2 H 2 O l - - H-571-6kJHeat of decomposition of water is -

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Enthalpy

2 H 2 g + O ...

Question

$2 H_{2 (g)} + O_{2 (g)} \to 2 H_{2} O_{(l)};$ $Δ H = - 571.6 k J$

Heat of decomposition of water is :

- 571.6 k J

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+ 571.6 k J

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- 1143.2 k J

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+ 285.8 k J

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Similar questions

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

Δ H = - 573.2 k J

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}

6 C (s) + 3 H_{2} (g) ⟶ C_{6} H_{6} (l), Δ H = 49.0 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l), Δ H = - 285.8 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g), Δ H = - 389.3 k J

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2 C_{4} H_{10} (g) + 13 O_{2} (g) ⟶ 8 C O_{2} (g) + 10 H_{2} O (l), Δ H = - 5757.2 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g), Δ H = - 405.4 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l), Δ H = - 572.4 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = - 393.7 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l)

Δ H = - 285.8 k J

C H_{3} C O O H (l) + 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (l)

Δ H = - 873.2 k J

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