Question 1

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

Accepted Answer

A) 15 g F2 
B) 15 g Ne 
C) 15 g Kr 
D) 15 g CO2 
E) All of these samples will have the same pressure. 
A) 15 g F2 
B) 15 g Ne 
C) 15 g Kr 
D) 15 g CO2 
E) All of these samples will have the same pressure.

Question 2

Rank the following in order of decreasing rate of effusion. F2 SF6 CO Kr

Accepted Answer

A) SF6 > Kr > F2 > CO 
B) Kr > CO > SF6 > F2 
C) F2 > Kr > CO > SF6 
D) CO > F2 > Kr > SF6 
E) CO > F2 > SF6 > Kr 
A) SF6 > Kr > F2 > CO 
B) Kr > CO > SF6 > F2 
C) F2 > Kr > CO > SF6 
D) CO > F2 > Kr > SF6 
E) CO > F2 > SF6 > Kr

Question 3

A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L)of gas will the syringe hold if 0.35 moles of Ne is added?

Accepted Answer

A) 0.87 L 
B) 4.9 L 
C) 1.2 L 
D) 2.1 L 
E) 1.9 L 
A) 0.87 L 
B) 4.9 L 
C) 1.2 L 
D) 2.1 L 
E) 1.9 L

Question 4

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mmHg, the level of mercury in the tube will

Accepted Answer

A) be 118 mm higher in the arm open to the atmosphere. 
B) be 118 mm higher in the arm connected to the gas cylinder. 
C) be 870 mm higher in the arm open to the atmosphere. 
D) be 870 mm higher in the arm connected to the gas cylinder. 
A) be 118 mm higher in the arm open to the atmosphere. 
B) be 118 mm higher in the arm connected to the gas cylinder. 
C) be 870 mm higher in the arm open to the atmosphere. 
D) be 870 mm higher in the arm connected to the gas cylinder.

Question 5

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 bar.

Accepted Answer

A) 63.1 K 
B) 5.25 K 
C) 337 K 
D) 28.0 K 
A) 63.1 K 
B) 5.25 K 
C) 337 K 
D) 28.0 K

Question 6

A sample of N2 effuses in 255 s. How long will the same size sample of Cl2 take to effuse?

Accepted Answer

A) 406 s 
B) 247 s 
C) 645 s 
D) 155 s 
E) 388 s 
A) 406 s 
B) 247 s 
C) 645 s 
D) 155 s 
E) 388 s

Question 7

How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the chemical equation shown below? Zn(s)+ 2HCl(aq)→ ZnCl2(aq)+ H2(g)

Accepted Answer

A) 0.171 g 
B) 5.76 g 
C) 11.7 g 
D) 131 g 
A) 0.171 g 
B) 5.76 g 
C) 11.7 g 
D) 131 g

Question 8

Convert 4744.1 mmHg to bar.

Accepted Answer

A) 7.549 bar 
B) 5.2423 bar 
C) 5.278 bar 
D) 6.817 bar 
E) 6.325 bar 
A) 7.549 bar 
B) 5.2423 bar 
C) 5.278 bar 
D) 6.817 bar 
E) 6.325 bar

Question 9

Give the major gas in dry air.

Accepted Answer

The answer of Give the major gas in dry air....

Question 10

Which of the following would have a density of 1.37 g L-1 at 7.0 °C and 0.9967 bar?

Accepted Answer

A) N2 
B) O2 
C) Kr  
D) Rn  
A) N2 
B) O2 
C) Kr  
D) Rn

Question 11

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N2 at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

Accepted Answer

A) 0.59 bar 
B) 1.1 bar 
C) 1.7 bar 
D) 1.9 bar 
E) 3.8 bar 
A) 0.59 bar 
B) 1.1 bar 
C) 1.7 bar 
D) 1.9 bar 
E) 3.8 bar

Question 12

Place the following gases in order of increasing density at STP. N2 NH3 N2O4 Ar

Accepted Answer

A) N2O4 2 3 
B) Ar 2O4 2 3 
C) N2 2O4 3 
D) NH3 2 2O4 
E) Ar 2 3 2O4 
A) N2O4 2 3 
B) Ar 2O4 2 3 
C) N2 2O4 3 
D) NH3 2 2O4 
E) Ar 2 3 2O4

Question 13

A gas mixture contains CO, Ar, and H2. What is the total pressure of the mixture if the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 bar?

Accepted Answer

A) 1.7 bar 
B) 0.20 bar 
C) 0.49 bar 
D) 0.60 bar 
E) 2.1 bar 
A) 1.7 bar 
B) 0.20 bar 
C) 0.49 bar 
D) 0.60 bar 
E) 2.1 bar

Question 14

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s-1 at 381 K.

Accepted Answer

A) 131 g mol-1 
B) 83.8 g mol-1 
C) 39.9 g mol-1 
D) 20.2 g mol-1 
E) 4.00 g mol-1 
A) 131 g mol-1 
B) 83.8 g mol-1 
C) 39.9 g mol-1 
D) 20.2 g mol-1 
E) 4.00 g mol-1

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

Rank the following in order of decreasing rate of effusion. F₂ SF₆ CO Kr

A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L)of gas will the syringe hold if 0.35 moles of Ne is added?

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mmHg, the level of mercury in the tube will

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 bar.

A sample of N₂ effuses in 255 s. How long will the same size sample of Cl₂ take to effuse?

How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the chemical equation shown below? Zn(s)+ 2HCl(aq)→ ZnCl₂(aq)+ H₂(g)

Convert 4744.1 mmHg to bar.

Give the major gas in dry air.

Which of the following would have a density of 1.37 g L^-1 at 7.0 °C and 0.9967 bar?

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N₂ at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

Place the following gases in order of increasing density at STP. N₂ NH₃ N₂O₄ Ar

A gas mixture contains CO, Ar, and H₂. What is the total pressure of the mixture if the mole fraction of H₂ is 0.35 and the pressure of H₂ is 0.58 bar?

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s^-1 at 381 K.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

Exam 5: Gases

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

Rank the following in order of decreasing rate of effusion. F2 SF6 CO Kr

A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L)of gas will the syringe hold if 0.35 moles of Ne is added?

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mmHg, the level of mercury in the tube will

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 bar.

A sample of N2 effuses in 255 s. How long will the same size sample of Cl2 take to effuse?

How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the chemical equation shown below? Zn(s)+ 2HCl(aq)→ ZnCl2(aq)+ H2(g)

Convert 4744.1 mmHg to bar.

Give the major gas in dry air.

Which of the following would have a density of 1.37 g L-1 at 7.0 °C and 0.9967 bar?

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N2 at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

Place the following gases in order of increasing density at STP. N2 NH3 N2O4 Ar

A gas mixture contains CO, Ar, and H2. What is the total pressure of the mixture if the mole fraction of H2 is 0.35 and the pressure of H2 is 0.58 bar?

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s-1 at 381 K.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallury

Transition Metals and Coordination Compounds

Filters

Rank the following in order of decreasing rate of effusion. F₂ SF₆ CO Kr

A sample of N₂ effuses in 255 s. How long will the same size sample of Cl₂ take to effuse?

How many grams of zinc metal are required to produce 2.00 L of hydrogen gas at STP according to the chemical equation shown below? Zn(s)+ 2HCl(aq)→ ZnCl₂(aq)+ H₂(g)

Which of the following would have a density of 1.37 g L^-1 at 7.0 °C and 0.9967 bar?

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N₂ at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP?

Place the following gases in order of increasing density at STP. N₂ NH₃ N₂O₄ Ar

A gas mixture contains CO, Ar, and H₂. What is the total pressure of the mixture if the mole fraction of H₂ is 0.35 and the pressure of H₂ is 0.58 bar?

Calculate the molecular weight of a gas that has a root mean square velocity of 269 m s^-1 at 381 K.