Answer
$-220.8\text{ kJ}$
Work Step by Step
$C_{(s)}+O_{2(g)}\Rightarrow CO_{2(g)}$ -397.3 kJ/mol Carbon
$2CO_{2(g)}\Rightarrow 2CO_{(g)}+O_{2(g)}$ 283.3 kJ/mol CO
Therefore,
$2C_{(s)}+2O_{2(g)}\Rightarrow 2CO_{2(g)}$ +
$2CO_{2(g)}\Rightarrow 2CO_{(g)}+O_{2(g)}$=
$2C_{(s)}+O_{2(g)}\Rightarrow 2CO_{(g)}$
and the enthalpy of the reaction is:
$2*(-393.7)+566.6=-220.8\text{ kJ}$
