How many grams of chlorine gas (Cl2) are in a 17.8 liter sample at 1.1 atmospheres and 29°C? Show all work used to solve this problem.

By using the ideal-gas equation: PV = nRT

where:

P = pressure = 1.1 atm

V = volume = 17.8 L

n = number of moles Cl2 (unknown)

R = gas constant = 0.08206 L*atm/mol*K

T = temperature = 29C + 273.15 = 302.15 K

To calculate number of moles of Cl2

(1.1 atm) * (17.8 L) = n * (0.08206 L*atm/mol*K) * (302.15 K)

n = 0.79 moles Cl2

Convert moles Cl2 to grams Cl2.

Note: 1 mole Cl2 = 70.9064 grams Cl2

0.79 moles Cl2 x (70.9064 grams Cl2/1 mole Cl2) = 56.0 grams Cl2