A 475 cm3 sample of gas at standard temperature (273 K) and pressure (1 atm) is allowed to expand until it occupies a volume of 600. cm3. What
temperature would be needed to return the gas to standard pressure (1 atm)?
(n = constant

T₂ =  344.8 K

Explanation:

Given data:

Initial volume of gas = 475 cm³

Initial temperature = 273 K

Final volume = 600 cm³

Final temperature = ?

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = T₁V₂/V₁  

T₂ = 273 K × 600 cm³ /  475 cm³

T₂ = 163800K . cm³ / 475 cm³

T₂ =  344.8 K

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.