Consider the reactionsCs - 2H2g - CH4g- - H - -x kcalCg-4Hg - CH4g- H - -x1 kcalCH4g - CH3g-Hg- H - -y kcalThe average bond energy of C - H bond in methane is

Consider the ...

Question

Consider the reactions
$C (s) + 2 H_{2} (g) ⟶ C H_{4} (g), Δ H = - x k c a l$
$C (g) + 4 H (g) ⟶ C H_{4} (g), Δ H = - x_{1} k c a l$
$C H_{4} (g) ⟶ C H_{3} (g) + H (g), Δ H = + y k c a l$
The average bond energy of $C - H$ bond in methane is

\frac{x}{4} k c a l m o l^{- 1}

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x_{1} k c a l m o l^{- 1}

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\frac{x_{1}}{4} k c a l m o l^{- 1}

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y k c a l m o l^{- 1}

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The enthalpy of atomisation for the reaction $C H_{4} (g) \to C (g) + 4 H (g) is 1665 k J m o l^{- 1}$ . What is the bond energy of C—H bond?

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

C H_{4}

⟶

C H_{4}

Δ

I . C H_{4} (g) \to C (g) + 4 H (g); Δ H = x_{1}

I I . C_{2} H_{6} (g) \to 2 C (g) + 6 H (g); Δ H = x_{2}

C (g) + 4 H (g) \to C H_{4} (g); Δ H = x k J

m o l^{- 1}

C (g r a p h i t e) + 2 H_{2} (g) \to C H_{4} (g); Δ H = y k J

m o l^{- 1}