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 1.00 L of 0.500 M NH4NO2 decomposes at 25.0°C?

First, let's find the number of moles of ammonium nitrite.

0.5 mol/L * 1.10 L = 0.6 mol

The decomposition reaction is

NH₄NO₂ → N₂ + 2 H₂O

Let's calculate the amount of N₂ gas produced.

0.6 mol * 1 mol N₂/1 mol NH₄NO₂ = 0.6 mol N₂

Then, let's compute P through the ideal gas equation:

P = nRT/V

P = (0.6) (0.0821 L-atm/mol-K) (25+273 K) / 10 L

P = 1.47 atm