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6.15 Calculate the enthalpy change for the process CCl4(g) → C(g) + 4 Cl(g) and calculate bond enthalpy of C ? Cl in CCl4(g). ΔvapH0(CCl4) = 30.5 kJ \mol?. ΔfH0 (CCl4) = ?135.5 kJ \mol?. ΔaH0 (C) = 715.0 kJ \mol? , where ΔaH0 is enthalpy of atomisation ΔaH0 (Cl2) = 242 kJ \mol?


6.15 Calculate the enthalpy change for the process


CCl4(g) → C(g) + 4 Cl(g)


and calculate bond enthalpy of C ? Cl in CCl4(g).


ΔvapH0(CCl4) = 30.5 kJ \mol?.


ΔfH0 (CCl4) = ?135.5 kJ \mol?.


ΔaH0 (C) = 715.0 kJ \mol? , where ΔaH0 is enthalpy of atomisation


ΔaH0 (Cl2) = 242 kJ \mol?


Grade:11

1 Answers

Aman Bansal
592 Points
12 years ago

Dear Student,

 

The chemical equations implying to the given values of enthalpies are:
 vapHθ = 30.5 kJ mol–1
  ΔaHθ = 715.0 kJ mol–1
  ΔaHθ = 242 kJ mol–1
 ΔfH = –135.5 kJ mol–1
Enthalpy change for the given process

Equation (ii) + 2 × Equation (iii) – Equation (i) – Equation (iv)
ΔH = ΔaHθ(C) + 2ΔaHθ (Cl2) – ΔvapHθ – ΔfH
= (715.0 kJ mol–1) + 2(242 kJ mol–1) – (30.5 kJ mol–1) – (–135.5 kJ mol–1)H = 1304 kJ mol–1
Bond enthalpy of C–Cl bond in CCl4 (g)
= 326 kJ mol–1

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