Given that- Cs - O2g- CO2g- - H - - 394 kJ 2H2g - O2g- 2H2Ol- - H - - 568 kJ CH4g - 2O2g- CO2g - 2H2Ol- - H - - 394 kJHeat of formation of CH4 is -

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Enthalpy of Combustion

Given that, ...

Question

Given that,
$C_{(s)} + O_{2 (g)} \to C O_{2 (g)};$ $Δ H = - 394 k J$
$2 H_{2 (g)} + O_{2 (g)} \to 2 H_{2} O_{(l)};$ $Δ H = - 568 k J$
$C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(l)};$ $Δ H = - 394 k J$
Heat of formation of $C H_{4}$ is :

-70 kJ

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71.8 kJ

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-244 kJ

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+782 kJ

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

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

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

{C H}_{3} O H (l)

{C H}_{3} O H (l) + \frac{3}{2} O_{2} (g) ⟶ C O_{2} (g) + 2 H_{2} O (l); Δ H = - 726 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 394 k J

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

C H_{3} O H (l)

C H_{3} O H (l) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l); △_{r} H^{⊖} = - 726 k J

C (s) + O_{2} (g) \to C O_{2} (g), Δ H = - 394 k J

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

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 ?)

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