Liquid nitrogen has a density of 0.807 g/ml at - 195.8 °c. if 1.00 l of n2 (l) is allowed to warm to 25°c at a pressure of 1.00 atm, what volume will the gas occupy? (r = 0.08206 l*atm/k*mol)

Step 1: Change density from g/mL to g/L;

0.807 g/mL = 807 g/L

Step 2: Find Moles of N₂;

As,

Density = Mass / Volume

Or,

Mass = Density * Volume

Putting Values,

Mass = 807 g/L * 1 L

Mass = 807 g

Also,

Moles = Mass / M. mass

Putting values,

Moles = 807 g / 28 g. mol⁻¹

Moles = 28.82 moles

Step 3: Apply Ideal Gas Equation to Find Volume of gas occupied,

As,

P V = n R T

V = n R T / P

Putting Values, remember! don't forget to change temperatue into Kelvin (25 °C + 273 = 298 K)

V = (28.82 mol * 0.08206 atm. L. mol⁻¹. K⁻¹ * 298 K) : 1 atm

V = 704.76 L