Question

Calculate the mass of 45.0 L of Cl₂ at

Answer 1

The mass of 45.0 L of Cl₂ at 87.0° C and 950 mm Hg is 134.7214 g.

Volume = 45.0 L

Temperature =  = (87.0 + 273) K = 360 K

Pressure = 950 mm Hg (1 mm Hg = 0.00131579 atm) = 1.25 atm

The formula used to calculate moles is as follows.

∴PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into the above formula as follows:

 ∴ PV = nRT

=> 1.25 atm × 45.0 L = n × 0.0821 L atm/mol K × 360K

=> n = 1.25 atm × 45.0 L / n × 0.0821 L atm/mol K × 360K

=> n = 56.25 / 29.556 mol

=> n = 1.90 mol

Moles is the mass of a substance divided by its molar mass. So, the mass of Cl₂ (molar mass = 70.906 g/mol) is calculated as follows:

∴  Moles = mass / molar mass

=> 1.90 mol = mass /  70.906 g/mol

=> mass = 134.7214 g

Thus, we can conclude that the mass of 45.0 L of Cl₂ at 87.0° C and 950 mm Hg is 134.7214 g.

To know more about the Ideal Gas Law :

brainly.com/question/28976906

Answer 2

Answer:

Don't follow this!

Explanation:

Your chemistry teacher knows that you are cheating and using this as your own work.

-From said teacher!