If the standard enthalpy change \(\left(\Delta_{\mathrm{r}} \mathrm{H}^\theta\right)\) for a certain reaction at \(298 \mathrm{~K}\) and constant pressure is \(-1860 \mathrm{~kJ}\) \(\mathrm{mol}^{-1}\), the standard entropy change \(\left(\Delta_{\text {sys }} \mathrm{s}^\theta\right)\) of the same reaction is \(-550 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\), which one of the following statements is correct?

1. A \(\left(\Delta_{\text {sys }} S^\theta\right)+\Delta_{\text {surr }} S^\theta=-7692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\), the reaction is spontaneous
2. B \(\left(\Delta_{\text {sys }} \mathrm{S}^\theta\right)+\Delta_{\text {surr }} \mathrm{S}^\theta=-5692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\), the reaction is non-spontaneous
3. C \(\left(\Delta_{\text {sys }} \mathrm{S}^\theta\right)+\Delta_{\text {surr }} \mathrm{S}^\theta=+5692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\), the reaction is spontaneous
4. D \(\left(\Delta_{\text {sys }} S^\theta\right)+\Delta_{\text {surr }} S^\theta=+7692 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\), the reaction is non-spontaneous