Question

A container of N2O3(g) has a pressure of 0.575 atm. When the absolute temperature of the N2O3(g) is tripled, the gas completely decomposes, producing NO2(g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change.

Answer 1

Answer:

3.45 atm

Step-by-step explanation:

Initial Pressure of N2O3 = 0.575

The pressure tripled for N2O3
So, 3x0.575=1.725

Then, N2O3 decomposes into NO2 and NO

N2O3–> NO2+NO

The pressure will double:
2x1.725=3.45

Therefore, the Final Pressure is:

3.45 atm