Answer:
Given:
(i) \[\text{CC}{{\text{l}}_{4}}(l)\to
CC{{l}_{4}}(g)\]\[\Delta {{H}^{{}^\circ }}=+30.5kJmo{{l}^{-1}}\]
(ii)
\[\Delta
{{H}^{{}^\circ }}=-135kJ\,mo{{l}^{-1}}\]
(iii) \[C(s)\to
C(g)\]\[\Delta {{H}^{{}^\circ }}=+715kJ\,mo{{l}^{-1}}\]
(iii) \[C{{l}_{2}}(g)\to
2Cl(g)\]\[\Delta {{H}^{{}^\circ }}=+242kJ\,mo{{l}^{-1}}\]
(iv)\[C{{l}_{2}}(g)\to
2Cl(g)\]\[\Delta {{H}^{{}^\circ }}=+242kJ\,mo{{l}^{-1}}\]
Required
equation
\[CC{{l}_{4}}(g)\to C(g)+4Cl(g)\]\[\Delta H=?\]
Equation
(iii) + 2 x Equation (iv) -Equation (ii) Equation (i) gives the required
equation
\[\Delta
H=715\text{ }+\text{ }2\left( 242 \right)\text{ }-30.5\text{ }-\left( -135.5
\right)\]
\[=1304\text{ }kJmo{{l}^{-1}}\]
Bond
enthalpy of \[(C-Cl)\]bond
\[=\frac{1304}{4}=326kJ\,mo{{l}^{-1}}\]
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