Given the enthalpy change for the reaction below:

$$\begin{array}{*{20}{l}} {{\text{2}}{{\text{H}}_{\text{2}}}{\text{(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \to {\text{2}}{{\text{H}}_{\text{2}}}{\text{O(l)}}}&{\Delta {H^\Theta } =  - 572{\text{ kJ}}} \end{array}$$

which statement is correct?

A.     The standard enthalpy change of combustion of ${{\text{H}}_2}{\text{(g)}}$ is $- 286{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}$.

B.     The standard enthalpy change of combustion of ${{\text{H}}_2}{\text{(g)}}$ is $+ 286{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}$.

C.     The standard enthalpy change of formation of ${{\text{H}}_2}{\text{O(l)}}$ is $- 572{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}$.

D.     The standard enthalpy change of formation of ${{\text{H}}_2}{\text{O(l)}}$ is $+ 572{\text{ kJ}}\,{\text{mo}}{{\text{l}}^{ - 1}}$.

A