Question 1

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas.What volume (L)of SO₂(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 × 10⁶ lb of this coal? (1 lb = 454 g)

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Question 2

Today is a beautiful day for a picnic in the mountains, so we seal our peanut butter sandwich in a plastic sandwich bag at the base of the mountain.The approximate volume of the sandwich bag not occupied by the sandwich is 200.mL.The pressure at the base of the mountain is 1.0 atm.If the pressure at the top of the mountain is 0.80 atm, what is the final volume (mL)of gas in our sandwich bag?

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Question 3

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final volume (mL)of the gas?

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Question 4

At STP, 1 mole of gas has a molar volume of 22.4 L.What is the density (g/L)of oxygen at STP?

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Question 5

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what was the initial volume (L)of the gas?

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Question 6

Give five examples (list names)of compounds that exist as gases at room temperature and pressure.

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Question 7

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final pressure (atm)of the gas?

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Question 8

At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L.How many moles of water vapor are present?

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Question 9

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is -5°C and the pressure is 1.0 millibar.What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.

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Question 10

In an effort to address concerns about global warming, a power plant in Portland,Oregon is designed to take all of its exhaust gases from its boilers and recycle the CO₂ using the Solvay process to make sodium hydrogen carbonate.The reaction is shown below. NH₃(g)+ H₂O(l)+ CO₂(g)+ NaCl(aq)$\rarr$NaHCO₃(aq)+ NH₄Cl(aq) How many liters each of NH₃ and CO₂ (both at STP)would be consumed to produce 3.00 kg of sodium bicarbonate?

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Question 11

Packaged cake mixes usually contain baking powder, a mixture of sodium hydrogen carbonate and calcium hydrogen phosphate that react to produce carbon dioxide gas when they are heated in water.The CO₂(g)formed allows the cake to "rise." When such cake mixes are used at high altitudes, often the cake will rise too much and collapse, unless special instructions are followed.Why does this happen?

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Question 12

What volume (L)of H₂ is formed at STP when 6.0 g of Al is treated with excess NaOH? 2NaOH + 2Al + 6H₂O $\rarr$ 2NaAl(OH)₄ + 3H₂(g)

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Question 13

A convenient way to produce very high purity oxygen in the laboratory is to decompose KMnO₄(s)at high temperature according to the following chemical equation: 2KMnO₄(s)$\rarr$K₂MnO₄(s)+ MnO₂(s)+ O₂(g) If 2.50 L of O₂(g)is needed at 1.00 atm and 20.°C, what mass (in grams)of KMnO₄(s)should be decomposed? Assume the decomposition of KMnO₄(s)goes to completion.

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Question 14

Baking powder is made up of sodium hydrogen carbonate and calcium hydrogen phosphate.When baking powder is wet, these components react to produce carbon dioxide.The equation for this reaction is given below. NaHCO₃(aq)+ CaHPO₄(aq)$\rarr$NaCaPO₄(aq)+ CO₂(g)+ H₂O(l) Assuming all of the carbon dioxide was released as a gas, how many liters of CO₂(g)would be formed at room temperature from 4.00 g of NaHCO₃ and excess CaHPO₄?

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Question 15

Give five examples (list names)of elements that occur as gases at room temperature and pressure?

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Question 16

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH₄NO₂(s)$\rarr$ N₂(g)+ 2H₂O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH₄NO₂ at 525°C and 1.5 atm?

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Question 17

Many automobiles produce about 5 grams of NO for each mile they are driven.How many liters of NO gas at STP would be produced on a 100-mile trip?

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Question 18

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final temperature (°C)of the gas?

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Question 19

At constant pressure, the density of a gas depends on temperature.Does the density increase or decrease as the temperature increases?

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Question 20

Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water.What volume (L)of oxygen at STP is necessary to react with 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL.1 gal = 3.78 L)

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Quiz 5: Gases

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas.What volume (L)of SO₂(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 × 10⁶ lb of this coal? (1 lb = 454 g)

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final volume (mL)of the gas?

At STP, 1 mole of gas has a molar volume of 22.4 L.What is the density (g/L)of oxygen at STP?

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what was the initial volume (L)of the gas?

Give five examples (list names)of compounds that exist as gases at room temperature and pressure.

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final pressure (atm)of the gas?

At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L.How many moles of water vapor are present?

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is -5°C and the pressure is 1.0 millibar.What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.

What volume (L)of H₂ is formed at STP when 6.0 g of Al is treated with excess NaOH? 2NaOH + 2Al + 6H₂O $\rarr$ 2NaAl(OH)₄ + 3H₂(g)

Give five examples (list names)of elements that occur as gases at room temperature and pressure?

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH₄NO₂(s) $\rarr$ N₂(g)+ 2H₂O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH₄NO₂ at 525°C and 1.5 atm?

Many automobiles produce about 5 grams of NO for each mile they are driven.How many liters of NO gas at STP would be produced on a 100-mile trip?

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final temperature (°C)of the gas?

At constant pressure, the density of a gas depends on temperature.Does the density increase or decrease as the temperature increases?

Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water.What volume (L)of oxygen at STP is necessary to react with 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL.1 gal = 3.78 L)

Quiz 5: Gases

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas.What volume (L)of SO2(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 × 106 lb of this coal? (1 lb = 454 g)

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final volume (mL)of the gas?

At STP, 1 mole of gas has a molar volume of 22.4 L.What is the density (g/L)of oxygen at STP?

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what was the initial volume (L)of the gas?

Give five examples (list names)of compounds that exist as gases at room temperature and pressure.

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final pressure (atm)of the gas?

At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L.How many moles of water vapor are present?

A gas-filled balloon with a volume of 12.5 L at 0.90 atm and 21°C is allowed to rise to the stratosphere where the temperature is -5°C and the pressure is 1.0 millibar.What is the final volume of the balloon in Liters? 1.000 atm = 1.013 bar.

What volume (L)of H2 is formed at STP when 6.0 g of Al is treated with excess NaOH? 2NaOH + 2Al + 6H2O →\rarr→ 2NaAl(OH)4 + 3H2(g)

Give five examples (list names)of elements that occur as gases at room temperature and pressure?

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH4NO2(s) →\rarr→ N2(g)+ 2H2O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH4NO2 at 525°C and 1.5 atm?

Many automobiles produce about 5 grams of NO for each mile they are driven.How many liters of NO gas at STP would be produced on a 100-mile trip?

The following data describes an initial and final state for an ideal gas.Given that the amount of gas does not change in the process, what is the final temperature (°C)of the gas?

At constant pressure, the density of a gas depends on temperature.Does the density increase or decrease as the temperature increases?

Gasoline (which can be considered to be octane, C8H18)burns in oxygen to produce carbon dioxide and water.What volume (L)of oxygen at STP is necessary to react with 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL.1 gal = 3.78 L)

A particular coal sample contains 2.32% S.When the coal is burned, the sulfur is converted to sulfur dioxide gas.What volume (L)of SO₂(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 × 10⁶ lb of this coal? (1 lb = 454 g)

What volume (L)of H₂ is formed at STP when 6.0 g of Al is treated with excess NaOH? 2NaOH + 2Al + 6H₂O $\rarr$ 2NaAl(OH)₄ + 3H₂(g)

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH₄NO₂(s) $\rarr$ N₂(g)+ 2H₂O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH₄NO₂ at 525°C and 1.5 atm?

Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water.What volume (L)of oxygen at STP is necessary to react with 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL.1 gal = 3.78 L)