Question

1. A light bulb is filled with 3.54 g of argon at 25 C and 725 mmHg. What is

the volume of this gas?

Answer 1

Answer: The volume of given gas is 2.27 L.

Step-by-step explanation:

Given: Mass = 3.54 g

Temperature =
`25^(o)C` = (25 + 273) K = 298 K

Pressure = 725 mm Hg (1 mm Hg = 0.00131579) = 0.95 atm

As moles is the mass of substance divided by its molar mass.

So, moles of argon (molar mass = 40 g/mol) is as follows.

`Moles = (mass)/(molar mass)\\= (3.54 g)/(40 g/mol)\\= 0.0885 mol`

Formula used to calculate the volume of given gas 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 above formula as follows.

`PV = nRT\\0.95 atm * V = 0.0885 mol * 0.0821 L atm/mol K * 298 K\\V = 2.27 L`

Thus, we can conclude that the volume of given gas is 2.27 L.