Use the References to access important values if needed for this question. Accor

Question

Use the References to access important values if needed for this question. According to the ideal gas law, a 09127 mol sample of nitrogen gas in a 1.628 L container at 270.5 K should exert a pressure of 12.44 atm. By what percent does the pressure calculated using the van der Wals equation differ fom the ideal pressure? For N, gas, a -1.390 L am mol 3.910x102 Umol. For N2 gas, a-1.390 L-atminol2 and b = Hint: % difference " 100x(P ideal . Pvan der Waals) / P ideal Retry Entire Group 8 more group attempts remaining Submit Answer

Explanation / Answer

Given that

Number of mole = 0.9127 mole T = 270.5 K

Pressure, P = 12.44 atm

V= 1.628 L

R = 0.0821L atm/Kmol
a = 1.390 L^2 atm/mol^2
b = 3.910*10^-2 OR 0.03910 L/mol

The Formula for P derived from Van der Waals Equation:
P = [nRT/(V - nb)] - n2a/V2

Substituting values:
P = {[(0.9127 *0.0821*270.5)] / [1.628-( 0.9127*0.03910)]} - [(0.9127^2* 1.390) / (1.628*2)]

P = (20.27/ 1.5923) – 0.437
P = 12.29 atm

% Difference = 100*[P ideal – P van der Waal ] / P ideal

= 100*[12.44 – 12.29 ] / 12.44

= 1.21%

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