Given Cs - O2g - CO2g - 94-2 Kcal H2g - 1-2O2g - H2Ol - 68-3 Kcal CH4g - 2O2g - CO2g - 2H2Ol-210-8 KcalThe heat of formation of methane in kcal will be-

The correct option is C 20 C+O_2→ CO_2+94.2 K cal . H_2+ 12 O_2→ H_2O +68.3 K cal . CH_4+ 2O_2→ CO_2+2 H_2O+ 210.8 K cal . C+O_2→ Co_2+94.2 K ...

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Methane

Given Cs + ...

Question

Given $C (s) + O_{2} (g) \to C O_{2} (g) + 94.2 K c a l$
$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) + 68.3 K c a l$
$C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l) + 210.8 K c a l$
The heat of formation of methane in kcal will be:

-45.9

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-47.8

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-20

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-47.3

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C (s) + O_{2} (g) \to C O_{2} (g) Δ H = + 94.2 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) + 68.3 Δ H = k c a l

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l) Δ H = + 210.8 k c a l

k c a l

C (s) + O_{2} (g) \to C O_{2} (g) Δ H = - 94.2 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) Δ H = - 68.3 k c a l

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l) Δ H = - 210.8 k c a l

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

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

25^{\circ} C

C H_{3} C O O H (l) + 2 O_{2} (g) \to 2 C O_{2} + 2 H_{2} O (l); Δ H = - 208.34

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.05

H_{2} (g) + \frac{1}{2} O_{2} \to H_{2} O (l); Δ H = - 68.32

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