Question
Asked Oct 4, 2019
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A 10.42 mol sample of methane gas is maintained in a 0.8003 L container at 302.3 K. What is the pressure in atm calculated using the van der Waals' equation for
a 2.253 L2atm/mol2 and b = 4.278x102 L/mol.
CH4 gas under these conditions? For CH4
atm
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A 10.42 mol sample of methane gas is maintained in a 0.8003 L container at 302.3 K. What is the pressure in atm calculated using the van der Waals' equation for a 2.253 L2atm/mol2 and b = 4.278x102 L/mol. CH4 gas under these conditions? For CH4 atm

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Expert Answer

Step 1

The vander Waals’ equation is given as

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n°a P+ (V-nb)=nRT v

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Step 2

For calculating the pressure of methane gas, the gi...

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Given, n 10.42 mol V=0.8003 L T 302.3 K a 2.253L atm/mol b 4.278x10 L/mol (10.42)x2.253 P+ |(0.8003-10.42x0.04278)=10.42 x0.0821x302.3 (0.8003) (P+381.93)(0.3545)=258 .6 1 P 347.6atm

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