1. Convert Temperature to Kelvin

* T(K) = T(°C) + 273.15

* T(K) = 20°C + 273.15 = 293.15 K

2. Use the Ideal Gas Law

* PV = nRT

* P = Pressure (atm) = 1 atm

* V = Volume (L) = 44 L

* n = Number of moles (mol)

* R = Ideal gas constant = 0.0821 L·atm/mol·K

* T = Temperature (K) = 293.15 K

3. Solve for n (moles)

* n = (PV) / (RT)

* n = (1 atm * 44 L) / (0.0821 L·atm/mol·K * 293.15 K)

* n ≈ 1.84 moles

Therefore, there are approximately 1.84 moles of N2 gas under these conditions.