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

Answer:

The answer to your question is        P = 1.357 atm

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

               $(P + \frac{a}{v^{2}} )(v - b) = RT$

Substitution

               $(P + \frac{0.211}{22.4})(22.4 - 0.0171) = (0.082)(373)$

Simplify

               (P + 0.0094)(22.3829) = 30.586

Solve for P

                           P + 0.0094 = $\frac{30.586}{22.3829}$

                           P + 0.0094 = 1.366

                                 P = 1.336 - 0.0094

                                P = 1.357 atm