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Bond Order and Enthalpy

CCl4g → Cg + ...

Question

$C C l_{4} (g) \to C (g) + 4 C (g)$
Calculate the bond enthalpy of $C - C l$ in $C C l_{4}$ .
$Δ H_{v a p} C C l_{4} = 30.5 K J m o l^{- 1}$
$Δ H_{f} C C l_{4} = - 135.5 K J m o l^{- 1}$
$Δ H_{a} C = 715.0 K J m o l^{- 1}$
$Δ H_{a} C l_{2} = 242 K J m o l^{- 1}$

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Solution

The chemical equations implying to the given values of enthalpies are:
(i) ${C C l_{4}}_{(l)} ⟶ {C C l_{4}}_{(g)}$ $Δ H_{v a p} : 30.5 k J / m o l$
(ii) $C_{(s)} ⟶ C_{(g)}$ $Δ H_{a} = 715.0 k J / m o l$
(iii) ${C l_{2}}_{(g)} ⟶ 2 C l_{(g)}$ $Δ H_{a} = 242 k J / m o l$
(iv) $C_{(g)} + {4 C l}_{(g)} ⟶ {C C l_{4}}_{(g)}$ $Δ H_{f} = - 135.5 k J / m o l$
Enthalpy change for the given process
${C C l_{4}}_{(g)} ⟶ C_{(g)} + 4 C l_{(g)}$
Equation (ii) $+ 2 \times$ Equation (iii) $-$ Equation (i) $-$ Equation (iv)
$= H = 1304 k J / m o l$
$∴$ Bond enthalpy of $C - C l$ bond in ${C C l_{4}}_{(g)} = \frac{1304}{4}$
$= 326 k J / m o l$

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Similar questions

Calculate the enthalpy change for the process

CCl₄₍_g₎ → C₍_g₎ + 4Cl₍_g₎

and calculate bond enthalpy of C–Cl in CCl₄₍_g_).

Δ_vapH^θ (CCl₄) = 30.5 kJ mol^–1.

Δ_fH^θ (CCl₄) = –135.5 kJ mol^–1.

Δ_aH^θ (C) = 715.0 kJ mol^–1, where Δ_aH^θ is enthalpy of atomisation

Δ_aH^θ (Cl₂) = 242 kJ mol^–1

Calculate the enthalpy change for the process

C C l_{4} (g) \to C (g) + 4 C l (g)

and calculate bond enthalpy of C-Cl in

C C l_{4} (g)

Δ_{v a p} H^{⊖} (C C l_{4}) = 30.5

^{- 1}

Δ_{f} H^{⊖} (C C l_{4}) = - 135.5

^{- 1}

Δ_{a} H^{⊖} (C) = 715.0

^{- 1}

Δ_{a} H^{⊖}

is enthalpy of atomisation

Δ_{a} H^{⊖} (C l_{2}) = 242

^{- 1}

△ H_{r}^{o}

for the reaction

C H_{2} C l_{2} (g) \to C (g) + 2 H (g) + 2 C l (g) .

The average bond enthalpies of C - H and C - Cl bonds are

414 k J m o l^{- 1}

330 k J m o l^{- 1} .

△ H_{r}^{o}

for the reaction

C H_{2} C l_{2} (g) \to C (g) + 2 H (g) + 2 C l (g) .

The average bond enthalpies of C - H and C - Cl bonds are

414 k J m o l^{- 1}

330 k J m o l^{- 1} .

Q. Calculate the bond energy of

C l - C l

bond from the following data:

C H_{4 (g)} + C l_{(g)} \to C H_{3} C l_{(g)} + H C l_{(g)}; Δ H = - 100.3 k J

. Also the bond enthalpies of

C - H, C - C l, H - C l

413, 326

431

k J m o l^{- 1}

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