What would be the change in pressure in a sealed 10.0 l vessel due to the formation of n2 gas when the ammonium nitrite in 1.40 l of 1.40 m nh4no2 decomposes at 25.0°c?

3.80 atm

Explanation:

First of all, ammonium nitrite decomposes to produce nitrogen gas and liquid water at the given room temperature:

Notice that the solid decomposes fully and produces the same number of moles of nitrogen:

Find moles of ammonium nitrite multiplying its molarity by its volume:

Express moles of nitrogen in terms of the ideal gas law:

Substitute the two expressions above into the molar ratio equation:

Solve for the pressure:

Notice that here R is the ideal gas law constant and we've converted the temperature into the absolute temperature: .

Therefore, the overall final pressure would be 4.80 atm. Since initially we had air in the vessel at standard conditions (1.00 atm), the change in pressure would be 4.80 atm - 1.00 atm = 3.80 atm.