5.E: Gases- Homework
Turn in your answers for the following questions - show your work
-
The volume of a bicycle tire is 1.35 liters and the manufacturer recommends a tire pressure of 125 PSI.
- If you want the bicycle tire to have the correct pressure at 20.0 °C, what volume of air is required at STP?
- If you fill the tire with nitrogen, what is the mass of the gas?
- You fill the bicycle tire to 125 PSI on a cold december day (-22 °F), and leave it until a hot day in July (101 °F). What is the pressure of the tire (assuming that it does not leak and it does not change volume or burst).
-
A fire extinguisher with a volume of 3.0 liters is filled with 150.0 grams of CO2.
- Assuming that it is an ideal gas, what is the pressure at 20.0 °C?
- What is the volume of the CO2 at 1.0 atm and 25 °C after the CO2 is released from the fire extinguisher?
-
A ballon used for sampling stratospheric ozone is filled with 150.0 kg of He. What is the volume of the balloon when,
- The balloon starts from a research station in Antartica at sea level where the barrometric pressure is 755 mmHg and the temperature is -25.0 °C.
- The balloon rises to 29,028 ft (8,848 m, the height of Mt Everest and about typical crusing altitude for a jet aircraft) the temperature is -70 °C and the pressure is 2.30x104 Pa.
- The balloon enters the stratosphere, at 65000 ft (20,000 m, crusing altutude for a U2 spy plane) the temperature is -70 °C and the pressure is 3.68x103 Pa.
The Following Questions are for your practice - Do Not Turn In. They include answers so you can check your work
Gas Pressure
-
A typical barometric pressure in Denver, Colorado, is 615 mm Hg. What is this pressure in atmospheres and kilopascals?
- answer
- 0.809 atm; 82.0 kPa
-
Consider this scenario and answer the following questions: On a mid-August day in the northeastern United States, the following information appeared in the local newspaper: atmospheric pressure at sea level 29.97 in., 1013.9 mbar.
- What was the pressure in kPa?
- The pressure near the seacoast in the northeastern United States is usually reported near 30.0 in. Hg. During a hurricane, the pressure may fall to near 28.0 in. Hg. Calculate the drop in pressure in torr.
- answer
- (a) 101.5 kPa; (b) 51 torr drop
Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
-
How would the graph in Figure change if the number of moles of gas in the sample used to determine the curve were doubled?
When a gas occupies a smaller volume, it exerts a higher pressure; when it occupies a larger volume, it exerts a lower pressure (assuming the amount of gas and the temperature do not change). Since P and V are inversely proportional, a graph of \(1/P\) vs. \( V\) is linear.- answer
- The curve would be farther to the right and higher up, but the same basic shape.
-
Determine the volume of 1 mol of CH
4
gas at 150 K and 1 atm, using
- answer
-
16.3 to 16.5 L
-
A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the pressure in the hot can?
- answer
-
3.40 × 10 3 torr
-
A weather balloon contains 8.80 moles of helium at a pressure of 0.992 atm and a temperature of 25 °C at ground level. What is the volume of the balloon under these conditions?
- answer
-
217 L
-
The effect of chlorofluorocarbons (such as CCl
2
F
2
) on the depletion of the ozone layer is well known. The use of substitutes, such as CH
3
CH
2
F(
g
), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:
- CCl 2 F 2 ( g )
- answer
-
(a) 1.85 L CCl 2 F 2
-
A balloon that is 100.21 L at 21 °C and 0.981 atm is released and just barely clears the top of Mount Crumpet in British Columbia. If the final volume of the balloon is 144.53 L at a temperature of 5.24 °C, what is the pressure experienced by the balloon as it clears Mount Crumpet?
- answer
-
0.644 atm
Stoichiometry of Gaseous Substances, Mixtures, and Reactions
-
A cylinder of O
2
(
g
) used in breathing by emphysema patients has a volume of 3.00 L at a pressure of 10.0 atm. If the temperature of the cylinder is 28.0 °C, what mass of oxygen is in the cylinder?
- answer
-
38.8 g
-
What is the molar mass of a gas if 0.0494 g of the gas occupies a volume of 0.100 L at a temperature 26 °C and a pressure of 307 torr?
- answer
-
1.) convert torr to atm and °C to °K
\(307\:torr=0.404atm\)
\(26°C= 300.°K\)
2.) Use the equation \(PV=nRT\) and solve for \(n\)
\(n=\dfrac{PV}{RT}\)
\(n=\dfrac{(0.404\:\cancel{atm})(0.100\:\cancel{L})}{(0.08206\dfrac{\cancel{atm}\:\cancel{L}}{mol\:\cancel{°K}})(300.\cancel{°K})}=0.00165\:moles\)
3.) Then divide grams by the number of moles to obtain the molar mass:
\(\dfrac{0.0494g}{0.00165\:moles}=30.0\dfrac{g}{mole}\)
-
Lime, CaO, is produced by heating calcium carbonate, CaCO
3
; carbon dioxide is the other product.
- Outline the steps necessary to answer the following question: What volume of carbon dioxide at 875° and 0.966 atm is produced by the decomposition of 1 ton (1.000 × 10 3 kg) of calcium carbonate?
- Answer the question.
- answer
-
(a) Balance the equation. Determine the grams of CO 2 produced and the number of moles. From the ideal gas law, determine the volume of gas. (b) 7.43 × 10 5 L
-
A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 torr. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)
- answer
-
XeF 2
Non-Ideal Gas Behavior
-
Graphs showing the behavior of several different gases follow. Which of these gases exhibit behavior significantly different from that expected for ideal gases?
- answer
-
Gases C, E, and F