Question 1

Which of the following statements is TRUE?

Accepted Answer

A)  Particles of different masses have the same average speed at a given temperature. 
B)  The larger a molecule, the faster it will effuse. 
C)  At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law. 
D)  For a given gas, the lower the temperature, the faster it will effuse. 
E)  None of the above statements is true. 
A)  Particles of different masses have the same average speed at a given temperature. 
B)  The larger a molecule, the faster it will effuse. 
C)  At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law. 
D)  For a given gas, the lower the temperature, the faster it will effuse. 
E)  None of the above statements is true.

Question 2

Which of the following samples will have the greatest average speed at 355 K?

Accepted Answer

A)  Kr 
B)  C2H4 
C)  Cl2 
D)  CH4 
E)  All of these samples will have the same average speed at the same temperature. 
A)  Kr 
B)  C2H4 
C)  Cl2 
D)  CH4 
E)  All of these samples will have the same average speed at the same temperature.

Question 3

How many liters of oxygen are needed to exactly react with 25.8 g of methane at STP? CH4(g)+ 2 O2(g)→ CO2(g)+ 2 H2O(l)

Accepted Answer

A)  18.1 L 
B)  36.2 L 
C)  72.3 L 
D)  78.9 L 
A)  18.1 L 
B)  36.2 L 
C)  72.3 L 
D)  78.9 L

Question 4

Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP).The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s)+ 2 CO2(g)→ 2 K2CO3(s)+ 3 O2(g)

Accepted Answer

A)  27.1 g, 80.4% yield 
B)  179 g, 12.2% yield 
C)  91.7 g, 23.8% yield 
D)  206 g, 10.6% yield 
E)  61.0 g, 35.7% yield 
A)  27.1 g, 80.4% yield 
B)  179 g, 12.2% yield 
C)  91.7 g, 23.8% yield 
D)  206 g, 10.6% yield 
E)  61.0 g, 35.7% yield

Question 5

Give the major gas in dry air.

Accepted Answer

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

Question 6

A mixture of 0.220 moles Rn,0.350 moles O2 and 0.640 moles Ar has a total pressure of 2.95 atm.What is the partial pressure of O2?

Accepted Answer

A)  1.17 atm 
B)  0.853 atm 
C)  1.03 atm 
D)  0.969 atm 
E)  0.649 atm 
A)  1.17 atm 
B)  0.853 atm 
C)  1.03 atm 
D)  0.969 atm 
E)  0.649 atm

Question 7

The density of nitric oxide (NO)gas at 1.35 atm and 29.8°C is ________ g/L.

Accepted Answer

A)  0.0543 
B)  0.614 
C)  1.63 
D)  0.552 
E)  16.6 
A)  0.0543 
B)  0.614 
C)  1.63 
D)  0.552 
E)  16.6

Question 8

A sample of N2 effuses in 200 s.How long will the same size sample of Cl2 take to effuse?

Accepted Answer

A)  318 s 
B)  126 s 
C)  507 s 
D)  78.9 s 
E)  388 s 
A)  318 s 
B)  126 s 
C)  507 s 
D)  78.9 s 
E)  388 s

Question 9

An instrument used to atmospheric pressure is called a

Accepted Answer

A)  barometer. 
B)  manometer. 
C)  sphygmomanometer. 
D)  spectrophotometer. 
E)  spectrometer. 
A)  barometer. 
B)  manometer. 
C)  sphygmomanometer. 
D)  spectrophotometer. 
E)  spectrometer.

Question 10

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

Accepted Answer

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

Question 11

What volume will 5.11 × 1022 atoms of Ne  occupy at STP?

Accepted Answer

A)  1.20 L 
B)  2.20 L 
C)  2.34 L 
D)  3.11 L 
E)  1.90 L 
A)  1.20 L 
B)  2.20 L 
C)  2.34 L 
D)  3.11 L 
E)  1.90 L

Question 12

A basketball is inflated to a pressure of 1.80 atm in a 23.0°C garage.What is the pressure of the basketball outside where the temperature is -2.00°C?

Accepted Answer

A)  1.65 atm 
B)  1.70 atm 
C)  1.90 atm 
D)  1.97 atm 
A)  1.65 atm 
B)  1.70 atm 
C)  1.90 atm 
D)  1.97 atm

Question 13

A compound is found to be 30.45% N and 69.55% O by mass.If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg,what is the molecular formula of the compound?

Accepted Answer

A)  NO2 
B)  N2O 
C)  N4O2 
D)  N2O5 
E)  N2O4 
A)  NO2 
B)  N2O 
C)  N4O2 
D)  N2O5 
E)  N2O4

Question 14

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 751 torr.Use Boyle's law to calculate the pressure (torr)when the volume is reduced to 9.25 L at a constant temperature of 25.0°C.

Accepted Answer

A)  812 torr 
B)  0.123 torr 
C)  6.95 ×   torr 
D)  695 torr 
E)  1.07 torr 
A)  812 torr 
B)  0.123 torr 
C)  6.95 ×   torr 
D)  695 torr 
E)  1.07 torr

Question 15

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.340 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below? H2O2(l)→ H2(g)+ O2(g)?

Accepted Answer

A)  402 mL 
B)  804 mL 
C)  1210 mL 
D)  1610 mL 
A)  402 mL 
B)  804 mL 
C)  1210 mL 
D)  1610 mL

Question 16

How many liters of hydrogen gas are needed to produce 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2(g)+ O2(g)→ 2 H2O(l)

Accepted Answer

A)  74.7 L 
B)  149 L 
C)  224 L 
D)  447 L 
A)  74.7 L 
B)  149 L 
C)  224 L 
D)  447 L

Question 17

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s)+     (aq)→ Zn   (aq)+   (g)
In an experiment,125 mL of wet   is collected over water at 27°C and a barometric pressure of   The vapor pressure of water at 27°C is 26.74 torr.The partial pressure of hydrogen in this experiment is ________ atm.

Accepted Answer

A)  0.955 
B)  726 
C)  0.991 
D)  780 
E)  1.03 
A)  0.955 
B)  726 
C)  0.991 
D)  780 
E)  1.03

Question 18

Define vapor pressure.

Accepted Answer

A)  partial pressure of water in a liquid mixture 
B)  partial pressure of water in a gaseous mixture 
C)  condensation of water 
D)  water dissolved in a liquid 
E)  water molecules 
A)  partial pressure of water in a liquid mixture 
B)  partial pressure of water in a gaseous mixture 
C)  condensation of water 
D)  water dissolved in a liquid 
E)  water molecules

Question 19

A 1.000 kg sample of nitroglycerine,C3H5N3O9,explodes and releases gases with a temperature of 1985°C at 1.000 atm.What is the volume of gas produced? 4 C3H5N3O9(s)→ 12 CO2(g)+ 10 H2O(g)+ 6 N2(g)+ O2(g)

Accepted Answer

A)  816.4 L 
B)  3878 L 
C)  5203 L 
D)  5916 L 
A)  816.4 L 
B)  3878 L 
C)  5203 L 
D)  5916 L

Question 20

A mixture of 8.0 mol Ne and 8.0 mol Xe are at STP in a rigid container.Which of the following statements is TRUE?

Accepted Answer

A)  Both gases have the same average kinetic energy. 
B)  Both gases contribute equally to the density of the mixture under these conditions. 
C)  Both gases have the same molecular speed. 
D)  The mixture has a volume of 22.4 L 
E)  All of the above are TRUE. 
A)  Both gases have the same average kinetic energy. 
B)  Both gases contribute equally to the density of the mixture under these conditions. 
C)  Both gases have the same molecular speed. 
D)  The mixture has a volume of 22.4 L 
E)  All of the above are TRUE.

Exam 5: Gases

Which of the following statements is TRUE?

Which of the following samples will have the greatest average speed at 355 K?

How many liters of oxygen are needed to exactly react with 25.8 g of methane at STP? CH4(g)+ 2 O2(g)→ CO2(g)+ 2 H2O(l)

Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP).The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s)+ 2 CO2(g)→ 2 K2CO3(s)+ 3 O2(g)

Give the major gas in dry air.

A mixture of 0.220 moles Rn,0.350 moles O2 and 0.640 moles Ar has a total pressure of 2.95 atm.What is the partial pressure of O2?

The density of nitric oxide (NO)gas at 1.35 atm and 29.8°C is ________ g/L.

A sample of N2 effuses in 200 s.How long will the same size sample of Cl2 take to effuse?

An instrument used to atmospheric pressure is called a

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

What volume will 5.11 × 1022 atoms of Ne occupy at STP?

A basketball is inflated to a pressure of 1.80 atm in a 23.0°C garage.What is the pressure of the basketball outside where the temperature is -2.00°C?

A compound is found to be 30.45% N and 69.55% O by mass.If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg,what is the molecular formula of the compound?

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 751 torr.Use Boyle's law to calculate the pressure (torr)when the volume is reduced to 9.25 L at a constant temperature of 25.0°C.

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.340 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below? H2O2(l)→ H2(g)+ O2(g)?

How many liters of hydrogen gas are needed to produce 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2(g)+ O2(g)→ 2 H2O(l)

Define vapor pressure.

A 1.000 kg sample of nitroglycerine,C3H5N3O9,explodes and releases gases with a temperature of 1985°C at 1.000 atm.What is the volume of gas produced? 4 C3H5N3O9(s)→ 12 CO2(g)+ 10 H2O(g)+ 6 N2(g)+ O2(g)

A mixture of 8.0 mol Ne and 8.0 mol Xe are at STP in a rigid container.Which of the following statements is TRUE?

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

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,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

How many liters of oxygen are needed to exactly react with 25.8 g of methane at STP? CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(l)

Determine the theoretical yield and the percent yield if 21.8 g of K₂CO₃ is produced from reacting 27.9 g KO₂ with 29.0 L of CO₂ (at STP).The molar mass of KO₂ = 71.10 g/mol and K₂CO₃= 138.21 g/mol. 4 KO₂(s)+ 2 CO₂(g)→ 2 K₂CO₃(s)+ 3 O₂(g)

A mixture of 0.220 moles Rn,0.350 moles O₂ and 0.640 moles Ar has a total pressure of 2.95 atm.What is the partial pressure of O₂?

A sample of N₂ effuses in 200 s.How long will the same size sample of Cl₂ take to effuse?

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

What volume will 5.11 × 10²²atoms of Ne occupy at STP?

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.340 grams of H₂O₂ at 700°C and 755 mm Hg according to the chemical equation shown below? H₂O₂(l)→ H₂(g)+ O₂(g)?

How many liters of hydrogen gas are needed to produce 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂(g)+ O₂(g)→ 2 H₂O(l)

A 1.000 kg sample of nitroglycerine,C₃H₅N₃O₉,explodes and releases gases with a temperature of 1985°C at 1.000 atm.What is the volume of gas produced? 4 C₃H₅N₃O₉(s)→ 12 CO₂(g)+ 10 H₂O(g)+ 6 N₂(g)+ O₂(g)