Consider the reaction 2NO₂(g) N₂O₄(g);$\Delta$H° = -56.8 kJ and $\Delta$S° = -175 J/K.In a container (at 298 K)N₂O₄(g)and NO₂(g)are mixed with initial partial pressures of 2.4 atm and 0.42 atm,respectively.Which of the following statements is correct?

Question

Quizplus · Accepted Answer

The negative value of ΔH° indicates that the reaction is exothermic and favors the formation of products. At the same time, the positive value of ΔS° indicates that the reaction favors disorder, which means that the reaction would be more favorable at higher temperatures. Since the reaction is exothermic, it is more likely that N₂O₄(g) will decompose into NO₂(g) rather than the reverse reaction. Therefore, the correct answer is A.

Consider the Reaction 2NO2(g) N2O4(g); Δ\DeltaΔ H° = -568 KJ And 2NO2(g)

Consider the Reaction 2NO₂(g) N₂O₄(g); $\Delta$ H° = -568 KJ And 2NO₂(g)