The heat of combustion of $C H_{4 (g)}, C_{(s)}$ and $H_{2 (g)}$ at $25^{o} C$ are -212.4 K cal, -94.0 K cal and -68.4 K cal respectively, the heat of formation of $C H_{4}$ will be:

+54.4 K cal

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-18.4 K cal

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-375.2 K cal

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+212.8 K cal

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Solution

The correct option is B -18.4 K cal
$c (s) + 2 H_{2} (g) \to C H_{4} Δ H_{F}$ =
$Δ H_{F} = {H c_{(c)} + 2 H C_{(H_{2})}} - {H C_{(C H_{a})}}$
= ${- 94 + 2 (- 68.4)} - {- 212.4}$
= -18.4 K cal

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The heat of combustion of CH4(g),C(s) and H2(g) at 25oC are -212.4 K cal, -94.0 K cal and -68.4 K cal respectively, the heat of formation of CH4 will be:

The correct option is B -18.4 K calc(s)+2H2(g)→CH4ΔHF = ΔHF={Hc(c)+2HC(H2)}−{HC(CHa)}= {−94+2(−68.4)}−{−212.4}= -18.4 K cal

The heat of combustion of $C H_{4 (g)}, C_{(s)}$ and $H_{2 (g)}$ at $25^{o} C$ are -212.4 K cal, -94.0 K cal and -68.4 K cal respectively, the heat of formation of $C H_{4}$ will be:

The correct option is B -18.4 K cal
$c (s) + 2 H_{2} (g) \to C H_{4} Δ H_{F}$ =
$Δ H_{F} = {H c_{(c)} + 2 H C_{(H_{2})}} - {H C_{(C H_{a})}}$
= ${- 94 + 2 (- 68.4)} - {- 212.4}$
= -18.4 K cal