Question

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.00 mol of neon gas at 100 °C is ________ atm. (a = 0.211 L2-atm/mol2, b = 0.0171 L/mol)

Answer 1

The answer to your question is P = 1.357 atm

Step-by-step explanation:

Data

Volume = 22.4 L

1 mol

temperature = 100°C

a = 0.211 L² atm

b = 0.0171 L/mol

R = 0.082 atmL/mol°K

Convert temperature to °K

Temperature = 100 + 273

= 373°K

Formula

`(P + (a)/(v^(2)) )(v - b) = RT`

Substitution

`(P + (0.211)/(22.4))(22.4 - 0.0171) = (0.082)(373)`

Simplify

(P + 0.0094)(22.3829) = 30.586

Solve for P

P + 0.0094 =
`(30.586)/(22.3829)`

P + 0.0094 = 1.366

P = 1.336 - 0.0094

P = 1.357 atm