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A certain balloon will pop if it expands to a volume greater than 16.0 L. The balloon is currently filled with air at a volume of 8.0 L. You heat the balloon such that the temperature measured in degrees Celsius doubles. Which of the following best describes what happens?


A) The balloon will expand to a volume greater than 16.0 L and pop.
B) The balloon will expand to a volume less than 16.0 L and not pop.
C) The balloon will expand to a volume of 16.0 L and pop.
D) The balloon will expand to a volume of 16.0 L and not pop.
E) The volume of the balloon will remain the same but the pressure will increase.

Correct Answer

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The air in the inner tube of the tire of a racing bike has a pressure of 116.8 psi. Convert this pressure to atm.


A) 0.1537 atm
B) 7.946 atm
C) 1717 atm
D) 1.153 atm
E) 116.8 atm

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Convert Convert atm to torr. A) torr B) 1.289 torr C) 68.1 torr D) torr E) torr atm to torr.


A) Convert atm to torr. A) torr B) 1.289 torr C) 68.1 torr D) torr E) torr torr
B) 1.289 torr
C) 68.1 torr
D) Convert atm to torr. A) torr B) 1.289 torr C) 68.1 torr D) torr E) torr torr
E) Convert atm to torr. A) torr B) 1.289 torr C) 68.1 torr D) torr E) torr torr

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Mercury vapor contains Hg atoms. What is the volume of 200. g of mercury vapor at 822 K and 0.415 atm?


A) 162 L
B) 27.9 L
C) 216 L
D) 108 L
E) 324 L

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An oxygen sample has a volume of 7.01 L at 27°C and 800.0 torr. How many oxygen molecules does it contain?


A) An oxygen sample has a volume of 7.01 L at 27°C and 800.0 torr. How many oxygen molecules does it contain? A) B) C) D) E) none of these
B) An oxygen sample has a volume of 7.01 L at 27°C and 800.0 torr. How many oxygen molecules does it contain? A) B) C) D) E) none of these
C) An oxygen sample has a volume of 7.01 L at 27°C and 800.0 torr. How many oxygen molecules does it contain? A) B) C) D) E) none of these
D) An oxygen sample has a volume of 7.01 L at 27°C and 800.0 torr. How many oxygen molecules does it contain? A) B) C) D) E) none of these
E) none of these

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Determine the pressure exerted by 2.26 mol of gas in a 2.92-L container at 32°C.


A) 2.03 atm
B) 56.6 atm
C) 19.4 atm
D) 5.93 atm
E) 17.3 atm

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A gas is collected over water at a certain temperature. The total pressure is 758 torr. The vapor pressure of water at this temperature is 17 torr. The partial pressure of the gas collected is


A) 758 torr
B) 17 torr
C) 775 torr
D) 741 torr
E) 733 torr

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You place 15.0 g of nitrogen gas and 15.0 g of hydrogen gas in a container fitted with a massless, frictionless piston. If the original volume of the container is 11.4 L, what is the volume after the reaction has run to completion? Assume constant temperature. N2(g) + 3H2(g) →\rightarrow 2NH3(g)


A) 13.17 L
B) 1.53 L
C) 7.09 L
D) 9.87 L
E) 1.32 L

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Perform the following conversion of pressure units: 0.875 atm = ____________ torr


A) 869
B) 88.6
C) 12.9
D) 665
E) 690

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D

How many liters of HCl(g) measured at STP can be produced from 5.44 g of Cl2 and excess H2 according to the following equation? How many liters of HCl(g) measured at STP can be produced from 5.44 g of Cl<sub>2</sub> and excess H<sub>2</sub> according to the following equation? A) 1.72 L B) 121.9 L C) 3.44 L D) 5.16 L E) none of these


A) 1.72 L
B) 121.9 L
C) 3.44 L
D) 5.16 L
E) none of these

Correct Answer

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A gas occupies 33.5 L at 2.00 atm pressure and 27°C. Calculate its volume at STP.


A) 73.6 L
B) 677 L
C) 30.5 L
D) 74.0 L
E) 61.0 L

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A 41.1-mL sample of H2 at STP would contain how many grams of hydrogen?


A) A 41.1-mL sample of H<sub>2</sub> at STP would contain how many grams of hydrogen? A) g B) 3.70 g C) 1.83 g D) g E) g g
B) 3.70 g
C) 1.83 g
D) A 41.1-mL sample of H<sub>2</sub> at STP would contain how many grams of hydrogen? A) g B) 3.70 g C) 1.83 g D) g E) g g
E) A 41.1-mL sample of H<sub>2</sub> at STP would contain how many grams of hydrogen? A) g B) 3.70 g C) 1.83 g D) g E) g g

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Consider a sample of gas in a container on a comfortable spring day in Chicago, IL. The Celsius temperature suddenly doubles, and you transfer the gas to a container with twice the volume of the first container. If the original pressure was 11 atm, what is a good estimate for the new pressure?


A) 12 atm
B) 2.8 atm
C) 5.9 atm
D) 11 atm
E) 22 atm

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Perform the following conversion of pressure units: 193 torr = ____________ atm


A) 1.91
B) 13.1
C) 0.254
D) 3.94
E) 953

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There are two balloons, both the same size and temperature. One balloon contains hydrogen and the other balloon contains carbon dioxide. The hydrogen balloon floats, and the carbon dioxide balloon sinks in the air. Which balloon contains a greater number of molecules?


A) The carbon dioxide balloon contains a greater number of molecules.
B) The hydrogen balloon contains a greater number of molecules.
C) Both balloons contain the same number of molecules.
D) This problem cannot be solved without more information given.

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C

Suppose a balloon has a maximum volume of 7.00 L. Also suppose each time you blow into a balloon, you expel 0.045 mol of air. How many times can you blow into the balloon before the balloon pops? Assume atmospheric conditions of 1.0 atm and 22°C and that your breath is at room temperature.

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We can blow into the...

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A 12.0-g sample of helium gas occupies a volume of 14.4 L at a certain temperature and pressure. What volume does a 24.0-g sample of neon occupy at these conditions of temperature and pressure?


A) 5.71 L
B) 28.8 L
C) 22.4 L
D) 36.3 L
E) 11.4 L

Correct Answer

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The largest a party balloon can get before bursting is 8.55 L at 25oC and 1.00 atm. Supposing you fill the balloon only with oxygen gas, how many grams of oxygen can be added to the balloon before it pops? Assume you have not yet added any gas to the balloon at all (so essentially the balloon is flat) .


A) 11.2 g O2
B) 0.350 g O2
C) 4.17 g O2
D) 133 g O2
E) 2.86 g O2

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A

You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.)


A) You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.) A) B) C) D) E)
B) You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.) A) B) C) D) E)
C) You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.) A) B) C) D) E)
D) You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.) A) B) C) D) E)
E) You have a partially filled party balloon with 2.00 g of helium gas. You then add 3.00 g of hydrogen gas to the balloon. Assuming constant temperature and pressure, how many times bigger is the party balloon - comparing before and after the hydrogen gas has been added. Choose the best formula to use to solve this problem. (V = volume of the gas, n = moles of the gas, m = mass of the gas, P = pressure of the gas.) A) B) C) D) E)

Correct Answer

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What volume of HCl(g) measured at STP can be produced from 1.91 g of H2 and excess Cl2 according to the following equation? What volume of HCl(g) measured at STP can be produced from 1.91 g of H<sub>2</sub> and excess Cl<sub>2</sub> according to the following equation? A) 21.2 L B) 42.4 L C) 86 L D) 173 L E) 64.2 L


A) 21.2 L
B) 42.4 L
C) 86 L
D) 173 L
E) 64.2 L

Correct Answer

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