Which of the following statements is true for the following reaction? NH₄HS(s)→ NH₃(g)+ H₂S(g); ΔH° = 93 kJ A)The reaction is not spontaneous at any temperature. B)The reaction is spontaneous only at relatively high temperatures. C)The reaction is at equilibrium under standard-state conditions. D)The reaction is spontaneous at all temperatures. E)The reaction is spontaneous only at relatively low temperatures.

Question

Quizplus · Accepted Answer

The reaction has a positive ΔH°, indicating it is endothermic, and the production of more moles of gas suggests an increase in entropy (ΔS° > 0). According to the Gibbs free energy equation (ΔG° = ΔH° - TΔS°), a positive ΔH° and positive ΔS° mean the reaction becomes more spontaneous at higher temperatures.

Which of the Following Statements Is True for the Following