Which of the following correctly represents the heat of formation of methane?

C (diamond) +

2 H_{2 (g)} \to C H_{4 (g)}

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C (diamond) +

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

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C (graphite) +

2 H_{2 (g)} \to C H_{4 (g)}

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C (graphite) +

4 H_{(g)} \to C H_{4 (g)}

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Solution

The correct option is B C (graphite) + $2 H_{2 (g)} \to C H_{4 (g)}$
By definition, the heat of formation of a compound is the heat evolved or absorbed when one mole of the compound is formed from its elements in their standard states. For carbon, the standard state is graphite.

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C H_{4}

C_{2} H_{4}

C (d i a m o n d) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H_{1}

C (g) + 4 H (g) ⟶ C H_{4} (g); Δ H_{2}

C (s) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H = - X k c a l

C (g) + 4 H (g) ⟶ C H_{4} (g); Δ H = - X_{1} k c a l

C H_{4} (g) ⟶ C H_{3} (g) + H (g); Δ H = + Y k c a l

C - H

(i) C_{(g)} + 4 H_{(g)} \to C H_{4 (g)}; △_{r} H = x k J m o l^{- 1} (i i) C (g r a p h i t e, s) + 2 H_{2 (g)} \to C H_{4 (g)}; △_{r} H = y k J m o l^{- 1}

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