What volume is occupied by 8.7 g of chlorine gas, Cl2, at 23°C and 1.15 atm pressure

V = 5.17L

Explanation:

Mass of gas = 8.7g

T = 23°C = (23 + 273.15) K = 296.15K

P = 1.15 atm

V = ?

R = 0.082atm. L / mol. K

From ideal gas equation

PV = nRT

P = pressure of the gas

V = volume of the gas

n = no. Of moles

R = ideal gas constant

T = temperature of the gas

no of moles = mass / molar mass

Molar mass of Chlorine = 35.5g / mol

No. Of moles = 8.7 / 35.5

No. Of moles = 0.245 moles

PV = nRT

V = nRT / P

V = (0.245 * 0.082 * 296.15) / 1.15

V = 5.9496 / 1.15

V = 5.17L

The volume of the gas is 5.17L