Question

According to the ideal gas law, a **10.08** mol
sample of **krypton** gas in a **0.8488**
L container at **496.7** K should exert a pressure of
**484.0** atm. By what percent does the pressure
calculated using the van der Waals' equation differ from the ideal
pressure? For **Kr** gas, a = **2.318**
L^{2}atm/mol^{2} and b =
**3.978×10 ^{-2}** L/mol.

----------------%

*Hint:* % difference = 100 × (P _{ideal} - P_{van
der Waals}) / P _{ideal}

Answer #1

PV = nRT

P = nRT/V

= 10.08*0.0821*496.7/0.8488 = 484atm

(P+an^2/V^2)(v-nb) = nRT

(P + 2.318*(10.08)^2/(0.8488)^2)(0.8488-10.08*0.03978) = 10.08*0.0821*496

(p + 326.9)(0.4478)= 410.4737

(P+326.9) = 916.64

P = 916.64-326.9 = 589.74

P = 589.74atm

% difference = 100 × (P _{VAN}- P_{IDEAL}) / P
_{VAN}

_{ }
= 100*(589.74-484)/589.74 = 17.92%

According to the ideal gas law, a 10.38 mol sample of krypton
gas in a 0.8420 L container at 502.0 K should exert a pressure of
507.8 atm. What is the percent difference between the pressure
calculated using the van der Waals' equation and the ideal
pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2
L/mol.

#25
A 10.86 mol sample of krypton
gas is maintained in a 0.7529 L container at
296.3 K. What is the pressure in atm calculated
using the van der Waals' equation for Kr gas under
these conditions? For Kr, a =
2.318L2atm/mol2 and b =
3.978×10-2 L/mol.
____atm
According to the ideal gas law, a 1.077 mol
sample of methane gas in a 1.670
L container at 265.4 K should exert a pressure of
14.05 atm. By what percent does...

According to the ideal gas law, a 10.59 mol
sample of argon gas in a 0.8229 L
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pressure? For Ar gas, a = 1.345
L2atm/mol2 and b =
3.219×10-2 L/mol.
??? %
Hint: % difference = 100 × (P ideal - Pvan
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Part 1 (5 points)
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Part 2 (5 points)
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If 1.00 mol of argon is placed in a 0.500-L container at 29.0 ∘C
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Use the van der Waals equation of state to calculate the
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P= ________ atm
Use the ideal gas equation to calculate the pressure under the
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P= ______ atm

Problem 18.41
For oxygen gas, the van der Waals equation of state achieves its
best fit for a=0.14N⋅m4/mol2 and
b=3.2×10−5m3/mol.
Part A
Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
volume is 0.50 L , calculated using the van der Waals equation.
Express your answer using two significant figures.
Part B
Determine the pressure in 1.7 mol of the gas at 9 ∘C if its
volume is 0.50 L , calculated using the ideal...

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