Question

13.0 moles of gas are in a 7.00L tank at 25.0?C . Calculate the
*difference* in pressure between methane and an ideal gas
under these conditions. The van der Waals constants for methane are
*a*=2.300L2?atm/mol2 and *b*=0.0430 L/mol.

Answer #1

A/c to ideal gas law

PV = nRT

ideal gas molecule behave likes a point particle and collison between them is prefectly elastic.

P= nRT/V

n=13, V=7L T= 273+25 =298 K

for ideal gas,

P= 13x0.0820x298 /7 =45.38 atm

Van der Wall's take into account moleculer size & moleculer interaction and gave aequation called Van der Wall equation which is given as

[P+a(n/V)^2](V/n-b)= RT

a=2.3 L2/atm/mol2 b= 0.043L/mol

[P+ 2.3(13/7)^2](7/13 -0.043) = 0.082x 298

[P+7.931](0.53846-0.043)=24.436

[P+7.931]= 24.436 / 0.49546=49.32

P= 49.32 - 7.931= 41.389 atm= Pressure of methane

Difference between pressure of ideal gas & methane gas

45.38 - 41.389 = 3.991 atm

13.0 moles of gas are in a 7.00 L tank at 20.5 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
Express your answer with the appropriate
units.

Part C
13.0 moles of gas are in a 5.00 L tank at 22.5 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
Express your answer with the appropriate units.
pressure difference =
Please enter pressure difference with Value and units.

15.0 moles of gas are in a 4.00 L tank at 21.2 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

12.0 moles of gas are in a 4.00 L tank at 24.4 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

12.0 moles of gas are in a 4.00 L tank at 21.6 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

15.0 moles of gas are in a 4.00 L tank at 20.1 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

14.0 moles of gas are in a 8.00 L tank at 21.0 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.

12.0 moles of gas are in a 5.00 L tank at 20.5 ∘C . Calculate
the difference in pressure between methane and an ideal gas under
these conditions. The van der Waals constants for methane are
a=2.300L2⋅atm/mol2 and b=0.0430 L/mol. Express your answer with the
appropriate units.

Part C
15.0 moles of gas are in a 3.00 L tank at 23.1 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
Express your answer with the appropriate units.
Hints
pressure difference =

15.0 moles of gas are in a 5.00 L tank at 23.1 ∘C . Calculate
the difference in pressure between methane and an ideal
gas under these conditions. The van der Waals constants for methane
are a=2.300L2⋅atm/mol2and b=0.0430 L/mol.
Express your answer with the appropriate units.

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