Answer:
26.99 % of air that will be displaced
Explanation:
Step 1: Data given
A 1.2-L container of liquid nitrogen is kept in a closet measuring 1.0m by 1.3m by 2.0m
Temperature = 23.5 °C
Atmospheric pressure = 1.2 atm
Liquid nitrogen has a density of 0.807 g/mL
Molar mass of N2 = 28 g/mol
Step 2: Calculate mass of nitrogen
Mass of nitrogen = density * volume
Mass of nitrogen = 0.807 g/mL * 1200 mL
Mass of nitrogen = 968.4 grams
Step 3: Calculate moles of N2
Moles N2 = mass N2 / molar mass N2
Moles N2 = 968.4 grams /28 g/mol
Moles N2 = 34.586 moles
Step 4: Calculate volume
p*V = n*R*T
⇒ p = the the pressure = 1.2 atm
⇒ V = the volume of N2 = TO BE DETERMINED
⇒ n = the number of moles = 34.586 moles
⇒ R = the gas constant = 0.08206 L*atm/K*mol
⇒ T = the temperature = 23.5 °C = 296.65
V = (n*R*T)/p
V = (34.586 * 0.08206 * 296.65)/1.2
V = 701.61 L
Step 5: Calculate the total volume of the chamber
1.0 m * 1.3 m * 2 m = 2.6 m³ = 2600 L
Step 6: Calculate the percent volume displaced
(701.61 L / 2600 L) * 100% = 26.99%
26.99 % of air that will be displaced
