Calculate the density of CO2(g)at 100°C and 10.0 atm pressure.

A) 1.44 g/L B) 134 g/L C) 44.0 g/L D) 53.6 g/L E) 14.4 g/L A) 1.44 g/L B) 134 g/L C) 44.0 g/L D) 53.6 g/L E) 14.4 g/L

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25°C.R = 0.08206 L.atm/K.mol.

A) 0.060 L B) 1.34 L C) 16.9 L D) 24.2 L E) 734 L A) 0.060 L B) 1.34 L C) 16.9 L D) 24.2 L E) 734 L

Exam 5: Gases | Examlex

Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water. What volume 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)

(Short Answer)

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Question 21

In a weather forecast on a Seattle radio station the barometric pressure was reported to be 29.4 inches.What is this pressure in SI units? (1 inch = 25.4 mm, 1 atm = 760 mmHg)

(Short Answer)

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Question 22

A spacecraft is filled with 0.500 atm of N₂ and 0.500 atm of O₂. Suppose a micrometeor strikes this spacecraft and puts a very small hole in it's side. Under these circumstances,

(Multiple Choice)

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Question 23

What is T in the table below?

(Short Answer)

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Question 24

A method of removing CO₂ from a spacecraft is to allow the CO₂ to react with sodium hydroxide. (The products of the reaction are sodium carbonate and water.)What volume of carbon dioxide at 25°C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts?

(Multiple Choice)

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Question 25

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO₂, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

(Multiple Choice)

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Question 26

What is the molar mass of Freon-11 gas if its density is 6.13 g/L at STP?

(Multiple Choice)

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Question 27

A sample of a gas occupies 1.40 *10³ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

(Multiple Choice)

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Question 28

What is the significance of the magnitude of the van der Waals "a" constant?

(Essay)

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Question 29

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? 1.000 atm = 1.013 bar.

(Short Answer)

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Question 30

If equal masses of O₂(g)and HBr(g)are in separate containers of equal volume and temperature, which one of these statements is true?

(Multiple Choice)

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Question 31

Give five examples of elements that occur as gases at room temperature and pressure?

(Essay)

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Question 32

Gas A and gas B are combined in a flask at initial pressures of 1.0 atm each.The flask is sealed and over time they react to completion to give gas C according to the following chemical equation: 2A(g)+ B(g) $\rarr$ C(g) Assuming the temperature stays constant, what will be the total pressure in the flask after the reaction goes to completion?

(Multiple Choice)

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Question 33

Calculate the density of N₂O gas, in grams per liter, at 110°C and 12 atm.

(Short Answer)

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Question 34

What is the pressure (in atmospheres)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

(Short Answer)

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Question 35

Calculate the density of CO₂(g)at 100°C and 10.0 atm pressure.

(Multiple Choice)

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Question 36

A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg.Identify the Noble gas in this sample? (R = 0.08206 L.atm/K.mol)

(Multiple Choice)

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Question 37

What is standard temperature and standard pressure?

(Short Answer)

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Question 38

Which of these properties is/are characteristic(s)of gases?

(Multiple Choice)

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Question 39

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25°C.R = 0.08206 L.atm/K.mol.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 109

Exam 5: Gases

Gasoline (which can be considered to be octane, C8H18)burns in oxygen to produce carbon dioxide and water. What volume 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)

In a weather forecast on a Seattle radio station the barometric pressure was reported to be 29.4 inches.What is this pressure in SI units? (1 inch = 25.4 mm, 1 atm = 760 mmHg)

A spacecraft is filled with 0.500 atm of N2 and 0.500 atm of O2. Suppose a micrometeor strikes this spacecraft and puts a very small hole in it's side. Under these circumstances,

What is T in the table below?

A method of removing CO2 from a spacecraft is to allow the CO2 to react with sodium hydroxide. (The products of the reaction are sodium carbonate and water.)What volume of carbon dioxide at 25°C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts?

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

What is the molar mass of Freon-11 gas if its density is 6.13 g/L at STP?

A sample of a gas occupies 1.40 *103 mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

What is the significance of the magnitude of the van der Waals "a" constant?

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? 1.000 atm = 1.013 bar.

If equal masses of O2(g)and HBr(g)are in separate containers of equal volume and temperature, which one of these statements is true?

Give five examples of elements that occur as gases at room temperature and pressure?

Calculate the density of N2O gas, in grams per liter, at 110°C and 12 atm.

What is the pressure (in atmospheres)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

Calculate the density of CO2(g)at 100°C and 10.0 atm pressure.

A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg.Identify the Noble gas in this sample? (R = 0.08206 L.atm/K.mol)

What is standard temperature and standard pressure?

Which of these properties is/are characteristic(s)of gases?

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25°C.R = 0.08206 L.atm/K.mol.

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

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Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

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Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

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Transition Metal Chemistry and Coordination Compounds

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Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water. What volume 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 spacecraft is filled with 0.500 atm of N₂ and 0.500 atm of O₂. Suppose a micrometeor strikes this spacecraft and puts a very small hole in it's side. Under these circumstances,

A method of removing CO₂ from a spacecraft is to allow the CO₂ to react with sodium hydroxide. (The products of the reaction are sodium carbonate and water.)What volume of carbon dioxide at 25°C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts?

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO₂, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

A sample of a gas occupies 1.40 *10³ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

If equal masses of O₂(g)and HBr(g)are in separate containers of equal volume and temperature, which one of these statements is true?

Calculate the density of N₂O gas, in grams per liter, at 110°C and 12 atm.

Calculate the density of CO₂(g)at 100°C and 10.0 atm pressure.

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25°C.R = 0.08206 L.atm/K.mol.