Question

What mass, in grams, of chlorine gas (Cl2) is contained in a 12.5-liter tank at 27.0 degrees Celsius and 2.85 atmospheres? Show all of the work used to solve this problem.

Answer 1

PV = nRT
P is pressure, V is volume, n is number of moles, R is the gas constant, T is temperature in K

(2.85 atm)(12.5 L) = (n)(.08206)(27 C + 273)

n = 1.45 moles x 35.45 grams / mol Cl2 = 51.3 grams

Answer 2

Answer: 101.367 grams of chlorine gas.

Explanation:

Pressure of the chlorine gas =P = 2.85 atm

Volume occupied by the gas = 12.5 L

Temperature of the gas = 27°C= 300 K (0°C = 273 K)

Number of moles of chlorine gas = n

PV = nRT

$2.85 atm\times 12.5 L=n\times 0.0820 L atm/K mol\times 300 K$

n = 1.4481 moles

Mass of the chlorine gas : 1.4481 moles × 70 g/mol = 101.367 g

101.367 grams of chlorine gas.