If the standard enthalpy change $\left({\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{H}}^{\ominus }\right)$ For a certain reaction at 298 K and constant pressure is $-1860\mathrm{kJ}{\mathrm{mol}}^{-1}$ , the standard entropy change $\left({\mathrm{\Delta }}_{\mathrm{sys}}{\mathrm{S}}^{\theta }\right)$ of the same reaction is $-550{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$, which one of the following statements is correct? 

$\left({\mathrm{\Delta }}_{\text{sys }}{\mathrm{S}}^{\ominus }\right)+{\mathrm{\Delta }}_{{\mathrm{\Delta }}_{\text{surr }}}{\mathrm{S}}^{\ominus }=+5692\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1},$the reaction is spontaneous

$\left({\mathrm{\Delta }}_{\text{sys }}{\mathrm{S}}^{\ominus }\right)+{\mathrm{\Delta }}_{{\mathrm{\Delta }}_{\text{surr }}}{\mathrm{S}}^{\theta }=-5692\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}$, the reaction is non- spontaneous

$\left({\mathrm{\Delta }}_{\text{sys }}{S}^{\theta }\right)+{\mathrm{\Delta }}_{\text{surr }}{S}^{\theta }=-7692\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}$, the reaction is spontaneous

$\left({\mathrm{\Delta }}_{\text{sys }}{\mathrm{S}}^{\theta }\right)+{\mathrm{\Delta }}_{{\mathrm{\Delta }}_{\text{surr }}}{\mathrm{S}}^{\theta }=+7692\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}$, the reaction is non- spontaneous