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) 16.7 L D) 24.2 L E) 734 L A) 0.060 L B) 1.34 L C) 16.7 L D) 24.2 L E) 734 L

Exam 5: Gases | Examlex

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)

(Short Answer)

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Question 61

What is the pressure (mmHg)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 742 mmHg and h = 16.7 cm?

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Question 62

At constant temperature, the volume of the container that a sample of nitrogen gas is in is doubled.As a result the pressure of the nitrogen gas is halved.The amount of nitrogen gas is unchanged in this process.This is an example of:

(Multiple Choice)

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Question 63

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63 °C and 745 mmHg.Identify the gas in the sample.(R = 0.08206 L.atm/K.mol)

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Question 64

At constant temperature and volume, a sample of oxygen gas is added to a sample of nitrogen gas.The pressure of the mixture is found by adding the pressures of the two individual gases.This is an example of:

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Question 65

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³.

(Multiple Choice)

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Question 66

Define Charles's Law

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Question 67

Calculate the volume of H₂(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

(Multiple Choice)

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Question 68

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm.If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

(Short Answer)

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Question 69

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 70

Phosgene, a chemical warfare agent used in World War I, consists of 12.41% C, 16.17% O, and 71.69% Cl.1.00 L of this gas at STP has a mass of 4.42 g.What is the molecular formula of phosgene?

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Question 71

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 72

A 45 mL sample of nitrogen gas is cooled from 135ºC to 15°C in a container that can contract or expand at constant pressure, what is the new volume of the nitrogen gas?

(Multiple Choice)

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Question 73

A 0.271 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg.The empirical formula of the compound is CH₂.What is the molecular formula of the compound?

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Question 74

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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Question 75

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

(Multiple Choice)

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Question 76

A 1.17 g sample of an alkane hydrocarbon gas occupies a volume of 674 mL at 28°C and 741 mmHg.Alkanes are known to have the general formula CnH2n+2.What is the molecular formula of the gas in this sample? (R = 0.08206 L.atm/K.mol)

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Question 77

Which of these gases will have the greatest density at the same specified temperature and pressure?

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Question 78

Determine the pressure of the gas trapped in the apparatus shown below when the atmospheric pressure is 695 mmHg.

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Question 79

A sample of hydrogen gas was collected over water at 21°C and 685 mmHg.The volume of the container was 7.80 L.Calculate the mass of H₂(g)collected.(Vapor pressure of water = 18.6 mmHg at 21°C.)

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Question 80

Showing 61 - 80 of 121

Exam 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)

What is the pressure (mmHg)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 742 mmHg and h = 16.7 cm?

At constant temperature, the volume of the container that a sample of nitrogen gas is in is doubled.As a result the pressure of the nitrogen gas is halved.The amount of nitrogen gas is unchanged in this process.This is an example of:

A 707 mg sample of a gas containing only carbon and oxygen occupies a volume of 452 mL at 63 °C and 745 mmHg.Identify the gas in the sample.(R = 0.08206 L.atm/K.mol)

At constant temperature and volume, a sample of oxygen gas is added to a sample of nitrogen gas.The pressure of the mixture is found by adding the pressures of the two individual gases.This is an example of:

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm3; the density of water is 1.00 g/cm3.

Define Charles's Law

Calculate the volume of H2(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm.If the can contains 1.0 g CO2 and is heated to 400°C, will it burst?

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.

Phosgene, a chemical warfare agent used in World War I, consists of 12.41% C, 16.17% O, and 71.69% Cl.1.00 L of this gas at STP has a mass of 4.42 g.What is the molecular formula of phosgene?

A 45 mL sample of nitrogen gas is cooled from 135ºC to 15°C in a container that can contract or expand at constant pressure, what is the new volume of the nitrogen gas?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg.The empirical formula of the compound is CH2.What is the molecular formula of the compound?

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

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

A 1.17 g sample of an alkane hydrocarbon gas occupies a volume of 674 mL at 28°C and 741 mmHg.Alkanes are known to have the general formula CnH2n+2.What is the molecular formula of the gas in this sample? (R = 0.08206 L.atm/K.mol)

Which of these gases will have the greatest density at the same specified temperature and pressure?

Determine the pressure of the gas trapped in the apparatus shown below when the atmospheric pressure is 695 mmHg.

A sample of hydrogen gas was collected over water at 21°C and 685 mmHg.The volume of the container was 7.80 L.Calculate the mass of H2(g)collected.(Vapor pressure of water = 18.6 mmHg at 21°C.)

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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)

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³.

Calculate the volume of H₂(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm.If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140.°C and 847 mmHg.The empirical formula of the compound is CH₂.What is the molecular formula of the compound?

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 sample of hydrogen gas was collected over water at 21°C and 685 mmHg.The volume of the container was 7.80 L.Calculate the mass of H₂(g)collected.(Vapor pressure of water = 18.6 mmHg at 21°C.)