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a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?   b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol.

a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?   b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter8: Properties Of Gases
Section8.7: Kinetic-molecular Theory And The Velocities Of Gas Molecules
Problem 8.12PSP
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a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?

 

b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol.

Express your answer to two significant figures and include the appropriate units.

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