If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?
- A$\Delta G = -50 \ kJ \ mol^{-1}$,the reaction is spontaneous
- B$\Delta G = -48.7 \ kJ \ mol^{-1}$,the reaction is non-spontaneous
- C$\Delta G = +50 \ kJ \ mol^{-1}$,the reaction is spontaneous
- D$\Delta G = +48.7 \ kJ \ mol^{-1}$,the reaction is non-spontaneous
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