🤓 Based on our data, we think this question is relevant for Professor Albright's class at UMICH.
Assume this reaction is carried out in the apparatus diagram below.
Nitric acid is produced commercially by the Ostwald process. In the first step, ammonium is oxidized to nitric oxide:
4 NH 3(g) + 5 O 2(g) → 4 NO(g) + 6 H 2O(g)
The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 3.00 L, and assume the temperature is constant.
1. 0.333 atm
2. 0.500 atm
3. 0.250 atm
4. 0.400 atm
5. 1.50 atm