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A) Calculate the pressure exerted by one mole of an ideal gas in a box that is 0.500 L and at 298 K.

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

B) Calculate the pressure of one mole of the following real gas in the same box at the same temperature: H2 (a=0.244 L2⋠atm/mol2, b=0.0266 L/mol).

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

C) Calculate the pressure of one mole of the following real gas in the same box at the same temperature: CH4 (a=2.25 L2⋠atm/mol2, b=0.0428 L/mol).

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

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Elin HesselLv2
28 Sep 2019
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Related questions

Part A) A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 22.0 ∘C is 2.55 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units.

Part B)

If 1.00 mol of argon is placed in a 0.500-L container at 26.0 ∘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)/mol2 and b=0.03219L/mol. Express your answer to two significant figures and include the appropriate units

If 1.00 mol of argon is placed in a 0.500-L container at 20.0 ∘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)/mol2 and b=0.03219L/mol. Enter the pressure difference in atmospheres using two significant figures.

Part A

A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 26.0?C is 2.05atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?

Express your answer to three significant figures and include the appropriate units.
mass of NH3 =

Part B

If 1.00 mol of argon is placed in a 0.500-L container at 29.0?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)/mol2 and b=0.03219L/mol.

Express your answer to two significant figures and include the appropriate units.
Pideal?Preal =

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