At high pressures, real gases do not behave ideally. calculate the pressure exerted by 18.0 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.

Part 1 (non-ideal behavior):

we will use Van der Waals formula:

P = (nRT / (V-nb)) - (n^2 a/V2)

when n (moles of H2) = 18 g / 2 = 9 moles

R (constant) = 0.0821

T (tempreature in kelvin = 20 + 273 = 293 K

V (Volume) = 1 L

a (constant for H2) = 0.2476

b (constant for H2) = 0.02661

So by substitution:

∴P = (9*0.0821*293 / (1 - (9*0.02661))) - (9^2*0.2476/1)

∴P ≈264.6 atm

Part 2 (ideal behavior):

we will use the ideal gas formula:

PV = nRT

when we have n = 9

R = 0.0821

T=293 K

V = 1 L

∴P = (9*0.0821*293) / 1 L

∴P = 216.5 atm