1) On a climb up Mt. Whitney, the atmospheric pressure is 511mmHg . Part A What
ID: 842746 • Letter: 1
Question
1) On a climb up Mt. Whitney, the atmospheric pressure is 511mmHg .
Part A
What is the pressure in atm?
P =___________ atm ?
Part B
What is the pressure in torr?
P = ________ torr ?
2) A 10.0L balloon contains He gas at a pressure of 650mmHg . What is the new pressure of the He gas at each of the following volumes if there is no change in temperature?
Part A
26.0L
P1 = ______mmHg
Part B
2.90L
P2 = ______mmHg
Part C
1000mL
P3 = ________ mmHg
3) A sample of methane (CH4) has a volume of 23mL at a pressure of 0.85atm . What is the volume, in milliliters, of the gas at each of the following pressures if there is no change in temperature and amount of gas?
Part A 0.10atm
Express your answer using three significant figures.
V1 = ____ mL
Part B 2.15atm
Express your answer using three significant figures.
V2 = _______mL
Part C 3500mmHg
Express your answer using three significant figures.
V3 = _______mL
4) A gas has a volume of 5.00L at 0?C. What final temperature, in degrees Celsius, is needed to change the volume of the gas to each of the following, if n and P do not change?
Part A 11.0L
Express your answer using two significant figures.
T1 = ______ ?C
Part B 1500mL
Express your answer using two significant figures.
T2 = _______ ?C
Part C 280L
Express your answer using two significant figures.
T3 = ______?C
Part D 76.5mL
Express your answer using three significant figures.
T4 = _____?C
5)
Part A
Use molar volume to find the number of grams of neon contained in 33.6L of Ne gas at STP.
Express your answer with the appropriate units.
mNe =
Part B
Use molar volume to find the number of grams of H2 contained in 1250mL of H2 gas at STP.
Express your answer with the appropriate units. mH2 =
6) In a gas mixture, the partial pressures are argon 430mmHg , neon 55mmHg , and nitrogen 165mmHg .
What is the total pressure (atm) exerted by the gas mixture?
P = ________ atm
7) A gas mixture containing oxygen, nitrogen, and neon exerts a total pressure of 1.40atm .
If helium added to the mixture increases the pressure to 1.90atm , what is the partial pressure (atm) of the helium?
Phelium = ______ atm
8) Calculate the new temperature, in degrees Celsius, for the following with n and V constant:
Part A
A sample of xenon at 30?C and 735mmHg is cooled to give a pressure of 615mmHg .
Express your answer to two significant figures and include the appropriate units.
T =
Part B
A tank of argon gas with a pressure of 0.955atm at -17?C is heated to give a pressure of 1260torr .
Express your answer to three significant figures and include the appropriate units.
T =
9)
Part A
A gas with an initial pressure of 1400torr at 165?C is cooled to 6?C
Pf = _____ torr
Part B
A gas in an aerosol can with an initial pressure of 1.25atm at 12?C is heated to 26?C.
Pf = ______ torr Solve for the new pressure, in torr, in each of the following, if n and V are constant.
10) A 80.0mL bubble of hot gases at 210?C and 1.74atm is emitted from an active volcano.
What is the new volume, in milliliters, of the bubble outside the volcano where the temperature is -30?C and the pressure is 0.80atm , if the amount of gas remains the same? V=
11) A weather balloon has a volume of 750L when filled with helium at 8?C at a pressure of 380torr .
What is the new volume of the balloon, where the pressure is 0.25atm and the temperature is -30?C .
V = _____ L
12) A scuba diver 40ft below the ocean surface inhales 85.0mL of compressed air from a scuba tank at a pressure of 2.60atm and a temperature of 5?C.
What is the pressure of the air, in atm, in the lungs when the gas expands to 185.0mL at a body temperature of 37?C, and the amount of gas remains constant?
P = _____ atm
13) Use molar volume to solve each of the following at STP.
Part A
The volume, in liters, occupied by 3.00moles of N2.
Express your answer using two significant figures.
V1 = ______ L
Part B
The volume, in milliliters, occupied by 0.420mole of He.
Express your answer using three significant figures.
V2 = _______mL
Explanation / Answer
1.PART A) 1 mmHg= 1/760atm
511 mmHg= 1/760*511 atm = 0.67 atm
P=0.67 atm
PART B) 1 mmHg= 1 torr
511 mmHg= 511 torr
P= 511 torr
2. 10.0L balloon contains He gas at a pressure= 650 mmHg
P1=650/10*26=1690 mmHg
P2=650/10*2.9=188.5 mmHg
P3=650/10*0.001 (1000mL=0.001L)
=0.065 mmHg
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