16 At constant T and P, a negative sign for ΔG indicates that(A)the reaction is exothermic.(B)the reaction is endothermic.(C)the reaction is fast.(D)the reaction is spontaneous.(E)ΔS must be＞0.

17 For the reaction H₂(g)+S(s)→H₂S(g), ΔH°=-20.2 kJ/mol and ΔS°=+43.1 J/K·mol. Which of these statements is true?(A)The reaction is only spontaneous at low temperatures.(B)The reaction is spontaneous at all temperatures.(C)ΔG° becomes less favorable as temperature increases.(D)The reaction is spontaneous only at high temperatures.(E)The reaction is at equilibrium at 25°C under standard conditions.

16 At constant T and P, a negative sign for ΔG indicates that

(A)the reaction is exothermic.

(B)the reaction is endothermic.

(C)the reaction is fast.

(D)the reaction is spontaneous.

(E)ΔS must be＞0.

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