A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet light from a burning magnesium strip. Then the following reaction occurs very rapidly: H2(g) + Cl2(g) → 2HCl(g) ΔG = –45.54 kJ ΔH = –44.12 kJ ΔS = –4.76 J/K Which of the following is consistent with this information? The reaction has a small equilibrium constant. The reaction is spontaneous, but the reactants are kinetically stable. The negative value for ΔS slows down the reaction. The ultraviolet light raises the temperature of the system and makes the reaction more favorable. The reactants are thermodynamically more stable than the products.