1.A cylinder with a moveable piston contains 0.504 molof gas and has a volume of

Question

1.A cylinder with a moveable piston contains 0.504 molof gas and has a volume of 278 mL .What will its volume be if an additional 0.178 mol of gas is added to the cylinder? (Assume constant temperature and pressure.)

2.

What is the volume occupied by 26.0 g of argon gas at a pressure of 1.47 atm and a temperature of 493 K ?A weather balloon is inflated to a volume of 29.2

3.L at a pressure of 744 mmHg and a temperature of 23.7 C. The balloon rises in the atmosphere to an altitude where the pressure is 395 mmHg and the temperature is -16.2 C.

Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

4.The following picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 .What would happen to the pressure if the volume were reduced to 0.5 L and the temperature increased to 260 C?

5.Use the molar volume of a gas at STP to calculate the density (in g/L) of oxygen gas at STP.

6.A sample of N2O gas has a density of 2.75 g/L at 298 K.What must be the pressure of the gas (in mmHg)?C

Explanation / Answer

1)At constant temp and pressure

v1/v2 = n1/n2

278/v2 = 0.504/0.682

v2 = 376.18ml

2) from ideal gas equation

pv = nRT (molar mass of argon is 39.9)

1.43*v = 26*0.0821*493/39.9

v= 18.44L

3) P1v1/T1 = P2v2/T2

744*29.2/296.7 = 395*v2/256.8

V2 = 47.60 L

4) use p1v1/T1 = P2v2/T2 ( Temperature i am not getting is dat 25? Or 250? Any way use formula to get answer

5)Since pv = nRT

p*molar mass = Density *RT

  at stp T=273k , p = 1atm

1*32 = Density *0.0821*273

density =1.427 g/L

6) P*molar mass = Density *RT

p*44 = 2.75*0.0821*298

P =1.529atm

1.529*760 =1162.12 Mm of hg

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

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