Answer:
Mass = 75.6 g
Explanation:
Given data:
Temperature of gas = 17°C
Volume of gas = 575 mL
Pressure of gas = 85000 mmHg
Mass of gas = ?
Solution:
Temperature of gas = 17°C (17+273 =290 K)
Volume of gas = 575 mL (575/1000 = 0.575 L)
Pressure of gas = 85000 mmHg (85000/760 = 111.8 atm)
Formula:
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
111.8 atm × 0.575 L = n×0.0821 atm.L/ mol.K × 290 K
64.285 atm. L = n×23.809 atm.L/ mol
n = 64.285 atm. L / 23.809 atm.L/ mol
n = 2.7 mol
Mass of nitrogen gas:
Mass = number of moles × molar mass
Mass = 2.7 mol × 28 g/mol
Mass = 75.6 g
