The thermal decomposition of dinitrogen pentoxide in the gas phase is represented by the equation
2 N₂O₅(g) → 4 NO₂(g) + O₂(g)
In a constant-volume container at 50 °C, the total pressure was measured at two times during the reaction.
• At t = 0 s, the pressure was 1.20 atm.
• At t = 600 s, the pressure had risen to 1.56 atm.
Assume all gases behave ideally and that the change in pressure is due solely to the reaction progress.
(a) Calculate the average rate of appearance of O₂(g) between 0 s and 600 s in units of atm s⁻¹.
(b) Express the rate from part (a) in mol L⁻¹ s⁻¹ for a container volume of 2.00 L at 50 °C. Show all reasoning, including any conversions used.
(c) Using your answer to part (b), determine the average rate of disappearance of N₂O₅(g) over the same time interval, clearly indicating the sign of the rate.