At high pressures, real gases do not behave ideally. calculate the pressure exerted by 25.0 g h2 at 20.0°c in a 1.00 l container assuming in part 1 non-ideal behavior and in part 2 ideal behavior.

Question

Parker Peck

Chemistry

26 August, 12:41

At high pressures, real gases do not behave ideally. calculate the pressure exerted by 25.0 g h2 at 20.0°c in a 1.00 l container assuming in part 1 non-ideal behavior and in part 2 ideal behavior.

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Nadia Freeman · Answer 1

Van der Waals equation is as follows:

(P + a (n/V) ²) * (V - nb) = n RT

Moles of H₂ is calculated by dividing 25 g by 2 (molecular weight of H₂) = 12.5 moles

Values of a and b are:

a = 0.02444 atm L² / mol

b = 0.0266 L / mol

(P + 0.02444 (12.5/1) ²) * (1 - (12.5 * 0.0266)) = 12.5 * 0.0821 * 293 K

If we solve this equation we get pressure of 412.29 atm

With ideal gas equation we get:

P V = n R T

P = n * R * T / V = (12.5 * 0.0821 * 293 / 1) = 300.69 atm