Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure meas

Question

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.

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.

Explanation / Answer

2.05 atm/ 1atm at STP * 3 L/22.4 L/mole at STP * (273)/(273 + 26) * 17 g/mole = 4.26grams

Here is part 2
Ideal gas law: PV=nRT
Van Der Waals: (P + (a/(V/n)^2)) ((V/n)-b)=RT
Ideal Pressure= nRT/V= 1mole x 0.082 L-atm/K-mole x 293K/.5L=48.1 atm
VDW: (P + (1.345/(.5/1)^2)) ((.5/1)-0.03219)= 0.082 x 293K
VDW: (P + 5.38) (.468)=24
0.468P + 2.52=24
0.468P=21.48
P=45.9 atm
Pideal-Preal= 48.1-45.9=2.2 atm

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.