At what temperature will a 1.00 g sample of neon gas exert a pressure of 500. torr in a 5.00 L container?

Answer 1

Hi Kz,

First we need to identify what variables we have and which variable we are looking for:

T = ? K

m = 1.00 g Ne

P = 500 Torr

V = 5.00 L

The formula that these variables match the most is: PV = nRT

P = pressure

Units: atm or torr

V = volume

Unit: L

n = moles

Unit: mol

R = gas constant

*0.08206 L•atm/mol•K

*62.36 L•torr/mol•K

*mainly two gas constants we use so make sure the units we have match the gas constant units

T = temperature

Unit: K (Kelvin)

We have most of these variables except for n (moles) so before we plug anything into the formula let’s convert m (mass) to n (moles):

1.00 g Ne • (1 mole Ne / 20.18 g Ne) = 0.04955 mole Ne

*note: 20.18 g is the molar mass of Ne

Now let’s plug in the variables we do have into the PV = nRT equation:

(500 torr)(5.00 L) = (0.04955 mol)(62.36 L•Torr/mol•K)(T)

*note: the gas constant units match the units we are given

*if we had the unit atm I would have chosen the other gas constant: 0.08206

Now solve for the variable T:

2500 = 3.0899•T

809.09 K = T

Answer: 809.09 K

Hope this helps :)