Consider this equation and the associated value for ${\mathrm{\Delta H}}^{\circ }$.

$2{\mathrm{H}}_2\left(\mathrm{g}\right)+2{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶4\mathrm{HCl}\left(\mathrm{g}\right); \mathrm{\Delta H}=-92.3\mathrm{kJ}$

Which statement about this information is incorrect?

If the equation is reversed. the ${\mathrm{\Delta H}}^{\circ }$ value equals +92.3 kJ.

The four $\mathrm{HCl}$ bonds are stronger than the four bonds in ${\mathrm{H}}_2$ and ${\mathrm{Cl}}_2$.

The ${\mathrm{\Delta H}}^{\circ }$ value will be -92.3 kJ if the $\mathrm{HCl}$ is produced as a liquid

23.1 kJ of heat will be evolved when 1 mol of $\mathrm{HCl}$(g) is produced.