I found out part 2 but I\'m somehow getting part 1 wrong O hups 8.5 out of 10 12

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I found out part 2 but I'm somehow getting part 1 wrong

O hups 8.5 out of 10 12/13/17 This is a Numeric Entry question/It is worth 1 point /You have unlimited attempts/There is no attempt penalty 10 Question (1 point) a See page 462 At high pressures, real gases do not behave ideally. Calculate the pressure exerted by 31.0 g H2 at 20.0°C in a 1.00L container assuming in Part 1 non ideal behavior and in Part 2 ideal behavior 4th attempt Part 1 (0.5 point) See Periodic Table See Hint Use the van der Waals equation and data in the hint to calculate the pressure exerted. 607.49 atm Part 2 (0.5 point) O See Hint Now, calculate the pressue excerted assuming that the gas behaves as an ideal gas. 372.86 atm 3rd attempt K 10/10 VIEW SOLUTION 8or e LIE N W A RE

Explanation / Answer

Mass of hydrogen = 31 gm

Molar mass =2 g/mole

Moles, n = 31/2= 15.5

Temperature, T= 20 deg.c =20+273= 293K

V= 1L

Vanderwal equation can be written as

(P+an2/v2)*(V-nb)= nRT

P= nRT/(V-nb)- an2/V2

R= 0.082057 L.atm/mole. K

for hydrogen, vanderwaal constants   are

a= 0.2453 bar.L2/mole2 and b= 0.02651 L/mole

substituting the values of n, R, T, a and b gives

P= 15.5*0.082057*293/(1-15.5*0.02651)- 0.2453*15.5*15.5/1

=573.6 bar

Using ideal gas law equation

P= nRT/V= 15.5*0.082057*293/1=372.6 bar

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