Answer: 56.0 g
Explanation:
1) Data:
mass, m = ?
Volume, V = 17.8 l
Pressure, P = 1.1 atm
Temperature, T = 29°C
molecule: Cl₂
2) Formulas:
i) ideal gas equation: PV = nRT
ii) m = n × molar mass
iii) molar mass = ∑ masses of all atoms in the chemical formula
3) Solution
i) n
n = PV / RT
R = universal constant of gases = 0.0821 atm×l / (K×mol)
T = 29 + 273.15 = 302.15K
n = [1.1 atm × 17.8 l ]/ [0.0821 atm×l / (k×mol) × 302.15 K] = 0.789 mol
ii) molar mass
Cl₂ ⇒ 2 × 35.5 g/mol = 71.0 g/mol
iii) mass in grams
mass = n × molar mass = 0.789 mol × 71.0 g/mol = 56.0 g
