Answer
$98.9\,kJ/mol$
Work Step by Step
$13.43\,g\,PbO=13.43\,g\,PbO\times\frac{1\,mol\,PbO}{223.2\,g\,PbO}=0.06017\,mol\,PbO$
$\Delta H$ for the reaction is the energy required to convert 1 mol PbO to lead.
Knowing that 5.95 kJ energy is required to convert $0.06017\,mol\,PbO$, we have
$\Delta H_{rxn}=\frac{5.95\,kJ}{0.06017\,mol}=98.9\,kJ/mol$
$\Delta H$ is positive as the energy is absorbed.
