Answer:
Information shadow:
The reaction is:
\[{{N}_{2}}{{O}_{4}}(g)+3CO(g)\to
{{N}_{2}}O(g)+3C{{O}_{2}}(g)\]
\[{{\Delta
}_{f}}H_{Co(g)}^{{}^\circ }=-110kJ\,mo{{l}^{-1}}\]
\[{{\Delta
}_{f}}H_{C{{O}_{2}}}^{{}^\circ }=-393kJmo{{l}^{-1}}\]
\[{{\Delta
}_{f}}H_{{{N}_{2}}O(g)}^{{}^\circ }=+81kJ\,mo{{l}^{-1}}\]
\[{{\Delta
}_{f}}H_{{{N}_{2}}{{O}_{4}}(g)}^{{}^\circ }=+9.7kJ\,mo{{l}^{-1}}\]
Problem
solving strategy:
\[{{\Delta
}_{r}}{{H}^{{}^\circ }}=\Sigma {{\Delta }_{f}}H_{\text{Products}}^{{}^\circ }-\Sigma
{{\Delta }_{f}}H_{\text{Reactants}}^{{}^\circ }\]
Working
it out:
\[{{\Delta
}_{r}}{{H}^{{}^\circ }}=[{{\Delta }_{f}}H_{{{N}_{2}}O(g)}^{{}^\circ }+3{{\Delta
}_{f}}H_{C{{O}_{2}}(g)}^{{}^\circ }]\]
\[-[{{\Delta
}_{f}}H_{{{N}_{2}}{{O}_{4}}(g)}^{{}^\circ }+3{{\Delta }_{f}}H_{CO(g)}^{{}^\circ
}]\]
\[=[81+3(-393)]-[9.7+3(-110)]=-777.7kJ\]
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