The pressure inside a hydrogen-filled container was 2.10.png”>at 21.png”>
The pressure inside a hydrogen-filled container was 2.10.png”>at 21.png”>
1-The pressure inside a hydrogen-filled container was 2.10.png”>at 21.png”>. What would the pressure be if the container was heated to 89.png”> ?
2-At standard temperature and pressure (0.png”>and 1.00.png”>), 1.00.png”>of an ideal gas occupies a volume of 22.4.png”>. What volume would the same amount of gas occupy at the same pressure and 95.png”> ?
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3- A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00.png”>and the initial pressure of chlorine was 1.90.png”> . The piston was pushed down to change the volume to 1.00.png”>. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.. (Figure 1)
4- A cylinder with a movable piston contains 2.00.png”>of helium,.png”>, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00.png”>to 2.50.png”> ? (The temperature was held constant.)
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5- At 4.00.png”>, an expandable vessel contains 0.864.png”>of oxygen gas. How many liters of oxygen gas must be added at constant temperature and pressure if you need a total of 1.84.png”> of oxygen gas in the vessel?
6- which of the following relationships are correct according to Boyle’s law?
1.png”>
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.png”> 2
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.png”> 3
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.png”> 4
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.png”> 5
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.png”> 6
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7-A certain gas is present in a 11.0.png”> cylinder at 2.0.png”> pressure. If the pressure is increased to 4.0.png”> the volume of the gas decreases to 5.5.png”> . Find the two constants.png”>, the initial value of.png”>, and.png”>, the final value of.png”>, to verify whether the gas obeys Boyle’s law.
8-If a certain gas occupies a volume of 20.png”> when the applied pressure is 10.png”> , find the pressure when the gas occupies a volume of 5.0.png”> .
9- How many air molecules are in a.png”>room? Assume atmospheric pressure of 1.00.png”>, a room temperature of 20.0.png”>, and ideal behavior.
10- Imagine that you have a 7.00.png”> gas tank and a 3.00.png”> gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 155.png”> , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.
11-What will the pressure inside the container become if the piston is moved to the 1.80.png”>mark while the temperature of the gas is kept constant?
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12-The gas sample has now returned to its original state of 1.00.png”>, 20.0.png”>and 1.00.png”>. What will the pressure become if the temperature of the gas is raised to 200.0.png”>and the piston isnot allowed to move?
13-The gas described in parts A and B has a mass of 1.66 grams. The sample is most likely which monoatomic gas?
14- When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction
.png”>
What is the mass of calcium carbonate needed to produce 57.0.png”> of carbon dioxide at STP?
15- Butane,.png”>, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is
.png”>
At 1.00.png”>and 23.png”>, what is the volume of carbon dioxide formed by the combustion of 3.80.png”> of butane?
16- Calculate the density of oxygen,.png”>, under each of the following conditions:
·STP
·1.00.png”>and 35.0.png”>
Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.
17-To identify a diatomic gas (.png”>), a researcher carried out the following experiment: She weighed an empty 1.7-.png”> bulb, then filled it with the gas at 1.20.png”> and 25.0.png”> and weighed it again. The difference in mass was 2.3.png”> . Identify the gas.
18- What is the partial pressure of argon,.png”>, in the flask?
1.png”> flask is filled with 1.45.png”> of argon at 25.png”>. A sample of ethane vapor is added to the same flask until the total pressure is 1.40.png”> .
19- What is the partial pressure of ethane,.png”>, in the flask?
20- In an effusion experiment, it was determined that nitrogen gas,.png”>, effused at a rate 1.812 times faster than an unknown gas. What is the molar mass of the unknown gas?
21- 15.0 moles of gas are in a 3.00.png”> tank at 20.0.png”> . Calculate thedifference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are.png”>and.png”>.
23-
Gas
.png”>
(.png”>)
.png”>
(.png”>)
.png”>
5.46
0.0305
.png”>
4.16
0.0373
.png”>
2.25
0.0428
.png”>
1.34
0.0322
Based on the given van der Waals constants, arrange these hypothetical gases in order of decreasing strength of intermolecular forces. Assume that the gases have similar molar masses.
24-To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 2.80.png”> of gas.png”>measured at 251.png”>in a 1.75-.png”> container assumingideal behavior?
25-To prevent tank rupture during deep-space travel, an engineering team is studying the effect of temperature on gases confined to small volumes. What is the pressure of 2.80.png”> of gas.png”>measured at 251.png”>in a 1.75-.png”> container assumingreal behavior?
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