Calculate urms, in m/s, for H2(g) molecules at 30°C.

A) 6.09 × 102 m/s B) 5.26 × 103 m/s C) 6.12 × 101 m/s D) 1.94 × 103 m/s E) 2.74 × 103 m/s A) 6.09 × 102 m/s B) 5.26 × 103 m/s C) 6.12 × 101 m/s D) 1.94 × 103 m/s E) 2.74 × 103 m/s

Consider the following reaction: N2(g) + 3 H2(g) → 2 NH3(g) What volume of NH3(g) can be produced from 200.0 L of H2(g) if the gases are measured at 350°C and 400 atm pressure?

A) 300.0 L B) 66.7 L C) 133.3 L D) 400.0 L E) 200.0 L A) 300.0 L B) 66.7 L C) 133.3 L D) 400.0 L E) 200.0 L

A sample of N2(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N2O2(g) to effuse under the same conditions?

A) 27.8 s B) 13.0 s C) 8.87 s D) 40.7 s E) 19.0 s A) 27.8 s B) 13.0 s C) 8.87 s D) 40.7 s E) 19.0 s

A gas of twice the molecular weight as CO2 will pass through a small hole how much faster than CO2?

A) 1/2 as fast B) 2 times as fast C) as fast D) (1/ ) as fast E) 4 times as fast A) 1/2 as fast B) 2 times as fast C) as fast D) (1/ ) as fast E) 4 times as fast

If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g), How much nitrogen is unreacted? All gases are at the same temperature and pressure.

A) 1.9 × 102 L B) 3.3 × 102 L C) 56 L D) 3.0 × 102 L E) 41 L A) 1.9 × 102 L B) 3.3 × 102 L C) 56 L D) 3.0 × 102 L E) 41 L

Exam 6: Gases | Examlex

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The volume in L H₂(g) (measured at 22°C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 °C and 760 mmHg) in the reaction 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l) is:

(Multiple Choice)

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Question 61

Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm³).

(Multiple Choice)

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Question 62

Calculate urms, in m/s, for H₂(g) molecules at 30°C.

(Multiple Choice)

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Question 63

Which of the following is a characteristic of an ideal gas?

(Multiple Choice)

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Question 64

The energy of molecules of a gas:

(Multiple Choice)

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Question 65

What volume would be occupied by a mixture of 0.33 g of hydrogen gas and 0.67 g of nitrogen gas at 157°C and 4.4 atm?

(Multiple Choice)

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Question 66

Liquid mercury freezes at a temperature of -39°C. The freezing point of mercury on the Kelvin scale is 234 K

(True/False)

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Question 67

Calculate the volume of H₂(g) expressed at STP, required to react with 3.00 L of CO(g) at STP in the following reaction: 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l)

(Multiple Choice)

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Question 68

To increase the volume of a fixed amount of gas from 100 cm3 to 200 cm3:

(Multiple Choice)

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Question 69

Consider the following reaction: N₂(g) + 3 H₂(g) → 2 NH₃(g) What volume of NH₃(g) can be produced from 200.0 L of H₂(g) if the gases are measured at 350°C and 400 atm pressure?

(Multiple Choice)

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Question 70

In the reaction 2 Na + 2 H₂O → 2 NaOH + H₂, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol)?

(Multiple Choice)

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Question 71

The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

(Multiple Choice)

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Question 72

A sample of N₂(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N₂O₂(g) to effuse under the same conditions?

(Multiple Choice)

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Question 73

How many liters of gas is 10.8 grams of nitrogen at 780 mmHg and 38.0°C?

(Multiple Choice)

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Question 74

The mutual attraction of gas molecules is an important aspect of:

(Multiple Choice)

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Question 75

A gas of twice the molecular weight as CO₂ will pass through a small hole how much faster than CO₂?

(Multiple Choice)

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Question 76

53.5 g of an ideal gas of molecular weight = 30.5 g/mol is confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.

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Question 77

The ideal gas equation connects three basic variables: volume, amount, and temperature of a gas.

(True/False)

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Question 78

If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃(g), How much nitrogen is unreacted? All gases are at the same temperature and pressure.

(Multiple Choice)

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Question 79

Butane (C₄H₁₀) is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?

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Question 80

Showing 61 - 80 of 100

Exam 6: Gases

The volume in L H2(g) (measured at 22°C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 °C and 760 mmHg) in the reaction 3 CO(g) + 7 H2(g) → C3H8(g) + 3 H2O(l) is:

Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3).

Calculate urms, in m/s, for H2(g) molecules at 30°C.

Which of the following is a characteristic of an ideal gas?

The energy of molecules of a gas:

What volume would be occupied by a mixture of 0.33 g of hydrogen gas and 0.67 g of nitrogen gas at 157°C and 4.4 atm?

Liquid mercury freezes at a temperature of -39°C. The freezing point of mercury on the Kelvin scale is 234 K

Calculate the volume of H2(g) expressed at STP, required to react with 3.00 L of CO(g) at STP in the following reaction: 3 CO(g) + 7 H2(g) → C3H8(g) + 3 H2O(l)

To increase the volume of a fixed amount of gas from 100 cm3 to 200 cm3:

Consider the following reaction: N2(g) + 3 H2(g) → 2 NH3(g) What volume of NH3(g) can be produced from 200.0 L of H2(g) if the gases are measured at 350°C and 400 atm pressure?

In the reaction 2 Na + 2 H2O → 2 NaOH + H2, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol)?

The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

A sample of N2(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N2O2(g) to effuse under the same conditions?

How many liters of gas is 10.8 grams of nitrogen at 780 mmHg and 38.0°C?

The mutual attraction of gas molecules is an important aspect of:

A gas of twice the molecular weight as CO2 will pass through a small hole how much faster than CO2?

53.5 g of an ideal gas of molecular weight = 30.5 g/mol is confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.

The ideal gas equation connects three basic variables: volume, amount, and temperature of a gas.

If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g), How much nitrogen is unreacted? All gases are at the same temperature and pressure.

Butane (C4H10) is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

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The volume in L H₂(g) (measured at 22°C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 °C and 760 mmHg) in the reaction 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l) is:

Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm³).

Calculate urms, in m/s, for H₂(g) molecules at 30°C.

Calculate the volume of H₂(g) expressed at STP, required to react with 3.00 L of CO(g) at STP in the following reaction: 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l)

Consider the following reaction: N₂(g) + 3 H₂(g) → 2 NH₃(g) What volume of NH₃(g) can be produced from 200.0 L of H₂(g) if the gases are measured at 350°C and 400 atm pressure?

In the reaction 2 Na + 2 H₂O → 2 NaOH + H₂, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol)?

A sample of N₂(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N₂O₂(g) to effuse under the same conditions?

A gas of twice the molecular weight as CO₂ will pass through a small hole how much faster than CO₂?

If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃(g), How much nitrogen is unreacted? All gases are at the same temperature and pressure.

Butane (C₄H₁₀) is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?