First slide

Hess law of constant summation

Question

$\large \frac{1}{2}{H_{2(g)}}\; + \;\frac{1}{2}C{l_{2(g)}}\; \to \;HC{l_{(g)}};\Delta {H^0} = \; - 92.4KJ/mole\$
$\large HC{l_{(g)}} + \;n{H_2}O\; \to H_{(aq)}^ + \;Cl_{_{(aq)}}^ - ;\Delta {H^0} = \; - 74.8KJ/mole\$
ΔH⁰f for Cl^-_(aq) is

Moderate

Solution

$\Delta H\; = \;\left[ {\Delta {H_{{H^ + }}}\; + \;\Delta {H_{C{l^ - }}}} \right]\; - \;\left[ {\Delta {H_{HCl}}} \right]$
-74.8=[O+ΔH_Cl_^-]-[-92.4]
-74.8= ΔH_Cl_^- +92.4
ΔH_Cl_^- =-74.8-92.4
= -167.2 KJ/mole

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