Find the temperature at which K_p = 4.00 for the reaction N₂O₄(g) 2NO₂(g).[Given: at 25°C, for NO₂(g), $\Delta$H°_f = 33.85 kJ/mol, S° = 240.46 J/mol·K; for N₂O₄(g), $\Delta$H°_f = 9.66 kJ/mol, S° = 304.3 J/mol·K; assume that$\Delta$H° and $\Delta$S° are independent of temperature.] A)197 °C B)56 °C C)36 °C D)79 °C E)476°C

Question

Quizplus · Accepted Answer

We can use the equation: ΔG° = ΔH° - TΔS° where ΔG° = -RTlnK_p and R = 8.314 J/mol·K. Rearranging, we get: T = (ΔH° - ΔG°)/ΔS° Substituting the given values, we get: T = (9.66 kJ/mol - (-RTln4.00))/304.3 J/mol·K At different temperatures, we can repeat this calculation by using the respective values of ΔH° and ΔS° from the given data. The temperature at which K_p = 4.00 will be the solution that matches the given choices. Calculating at 25°C (298 K): T = (9.66 kJ/mol - (-8.314 J/mol·K x ln4.00))/304.3 J/mol·K T = 79°C Therefore, the correct answer is D) 79°C.

Find the Temperature at Which Kp = 4 Δ\DeltaΔ H°f = 33

Find the Temperature at Which K_p = 4 $\Delta$ H°_f = 33