Calculate the density of Br2(g) at 59.0$\circ$C and 1.00 atm pressure.

A) 3.45 g/L B) 5.83 g/L C) 22.4 g/L D) 27.2 g/L E) 769 g/L A) 3.45 g/L B) 5.83 g/L C) 22.4 g/L D) 27.2 g/L E) 769 g/L

How many liters of chlorine gas at 25$\circ$C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 with excess HCl(aq) according to the following chemical equation MnO2(s) + 4HCl(aq) $\rarr$MnCl2(aq) + 2H2O(l) + Cl2(g)

A) 5.36 * 10-3 L B) 0.138 L C) 0.282 L D) 3.09 L E) 3.55 L A) 5.36 * 10-3 L B) 0.138 L C) 0.282 L D) 3.09 L E) 3.55 L

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.$\circ$C, what mass (in grams) of KMnO4(s) should be decomposed Assume the decomposition of KMnO4(s) goes to completion.

A) 35.8 g B) 34.8 g C) 33.8 g D) 32.8 g E) None of the above A) 35.8 g B) 34.8 g C) 33.8 g D) 32.8 g E) None of the above

Calculate the grams of SO2 gas present at STP in a 5.9 L container.

A) 0.24 g B) 0.26 g C) 15 g D) 17 g E) 64 g A) 0.24 g B) 0.26 g C) 15 g D) 17 g E) 64 g

Calculate the density of CO2(g) at 120$\circ$C and 790 mmHg pressure.

A) 0.032 g/L B) 1.4 g/L C) 1.8 g/L D) 3.4 g/L E) 8.0 g/L A) 0.032 g/L B) 1.4 g/L C) 1.8 g/L D) 3.4 g/L E) 8.0 g/L

Exam 5: Gases | Examlex

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28^$\circ$C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28^$\circ$C is 28.3 mmHg.

(Multiple Choice)

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Question 61

Boyle's Law states that the volume of a fixed amount of gas maintained at constant temperature is directly proportional to the gas pressure

(True/False)

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Question 62

Which of the following is not an example of a compound that exists as a gas at room temperature and pressure.

(Multiple Choice)

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Question 63

Calculate the density of Br₂(g) at 59.0^$\circ$C and 1.00 atm pressure.

(Multiple Choice)

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Question 64

The gas pressure in an aerosol can is 1.8 atm at 25^$\circ$C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475^$\circ$C

(Multiple Choice)

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Question 65

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)

(Multiple Choice)

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Question 66

How many liters of chlorine gas at 25^$\circ$C and 0.950 atm can be produced by the reaction of 12.0 g of MnO₂ with excess HCl(aq) according to the following chemical equation MnO₂(s) + 4HCl(aq) $\rarr$ MnCl₂(aq) + 2H₂O(l) + Cl₂(g)

(Multiple Choice)

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Question 67

What will happen to the height (h) of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg

(Multiple Choice)

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Question 68

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.^$\circ$C, what mass (in grams) of KMnO₄(s) should be decomposed Assume the decomposition of KMnO₄(s) goes to completion.

(Multiple Choice)

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Question 69

A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25^$\circ$C. One now finds that the gas pressure inside the container is 1.73 atm. What mass of mercury(II) oxide was originally placed into the container

(Multiple Choice)

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Question 70

Calculate the grams of SO₂ gas present at STP in a 5.9 L container.

(Multiple Choice)

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Question 71

1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0^$\circ$C. What is the molar mass of Freon-113

(Multiple Choice)

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Question 72

0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure. What is the volume of 0.125 mol of this gas at the same temperature and pressure

(Multiple Choice)

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Question 73

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

(Multiple Choice)

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Question 74

Calculate the density of CO₂(g) at 120^$\circ$C and 790 mmHg pressure.

(Multiple Choice)

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Question 75

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 76

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4^$\circ$C and 3.0 atm, to the water's surface, where the temperature is 25^$\circ$C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

(Multiple Choice)

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Question 77

10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final gas pressure inside the vessel at 23ºC

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Question 78

Which one of these gases is "lighter-than-air"

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Question 79

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^$\circ$C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts

(Multiple Choice)

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Question 80

Showing 61 - 80 of 130

Exam 5: Gases

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28 ∘\circ∘ C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28 ∘\circ∘ C is 28.3 mmHg.

Boyle's Law states that the volume of a fixed amount of gas maintained at constant temperature is directly proportional to the gas pressure

Which of the following is not an example of a compound that exists as a gas at room temperature and pressure.

Calculate the density of Br2(g) at 59.0 ∘\circ∘ C and 1.00 atm pressure.

The gas pressure in an aerosol can is 1.8 atm at 25 ∘\circ∘ C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475 ∘\circ∘ C

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)

How many liters of chlorine gas at 25 ∘\circ∘ C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 with excess HCl(aq) according to the following chemical equation MnO2(s) + 4HCl(aq) →\rarr→ MnCl2(aq) + 2H2O(l) + Cl2(g)

What will happen to the height (h) of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg

Calculate the grams of SO2 gas present at STP in a 5.9 L container.

1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0 ∘\circ∘ C. What is the molar mass of Freon-113

0.820 mole of hydrogen gas has a volume of 2.00 L at a certain temperature and pressure. What is the volume of 0.125 mol of this gas at the same temperature and pressure

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

Calculate the density of CO2(g) at 120 ∘\circ∘ C and 790 mmHg pressure.

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.

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4 ∘\circ∘ C and 3.0 atm, to the water's surface, where the temperature is 25 ∘\circ∘ C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final gas pressure inside the vessel at 23ºC

Which one of these gases is "lighter-than-air"

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 ∘\circ∘ C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts

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A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28^$\circ$C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28^$\circ$C is 28.3 mmHg.

Calculate the density of Br₂(g) at 59.0^$\circ$C and 1.00 atm pressure.

The gas pressure in an aerosol can is 1.8 atm at 25^$\circ$C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 475^$\circ$C

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)

How many liters of chlorine gas at 25^$\circ$C and 0.950 atm can be produced by the reaction of 12.0 g of MnO₂ with excess HCl(aq) according to the following chemical equation MnO₂(s) + 4HCl(aq) $\rarr$ MnCl₂(aq) + 2H₂O(l) + Cl₂(g)

Calculate the grams of SO₂ gas present at STP in a 5.9 L container.

1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0^$\circ$C. What is the molar mass of Freon-113

Calculate the density of CO₂(g) at 120^$\circ$C and 790 mmHg pressure.

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.

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4^$\circ$C and 3.0 atm, to the water's surface, where the temperature is 25^$\circ$C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

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^$\circ$C and 749 mmHg can be removed per kilogram of sodium hydroxide that reacts