Question 1

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl2 at 325 K.What is the partial pressure of Cl2?

Accepted Answer

A)  16.0 atm 
B)  19.5 atm 
C)  6.53 atm 
D)  35.5 atm 
A)  16.0 atm 
B)  19.5 atm 
C)  6.53 atm 
D)  35.5 atm

Question 2

A sample of CO2 gas fills a container with a volume of 44.5 L.When the volume is decreased to 13.8 L at a constant temperature,the pressure inside the container is 6.25 atm.What was the pressure inside the container originally?

Accepted Answer

A)  0.035 atm 
B)  0.51 atm 
C)  1.94 atm 
D)  3.84 atm 
E)  6.25 atm 
A)  0.035 atm 
B)  0.51 atm 
C)  1.94 atm 
D)  3.84 atm 
E)  6.25 atm

Question 3

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 are 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 are true.

Question 4

The mole fraction of argon in dry air near sea level is 1.818 × 10-5 where the molar mass of argon is 39.948.The concentration of argon in the atmosphere is ________ ppm.

Accepted Answer

A)  1.07 × 108 
B)  0.934 
C)  9.34 × 106 
D)  18.18 
E)  9.34 × 109 
A)  1.07 × 108 
B)  0.934 
C)  9.34 × 106 
D)  18.18 
E)  9.34 × 109

Question 5

Why does hot air rise?

Accepted Answer

As air is heated,it expands an

Question 6

The density of chlorine gas at 1.21 atm and 34.9°C is ________ g/L.

Accepted Answer

A)  0.0479 
B)  0.295 
C)  0.423 
D)  1.70 
E)  3.39 
A)  0.0479 
B)  0.295 
C)  0.423 
D)  1.70 
E)  3.39

Question 7

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm.What is the identity of the halogen?

Accepted Answer

A)  Br2 
B)  F2 
C)  Cl2 
D)  I2 
E)  Ge 
A)  Br2 
B)  F2 
C)  Cl2 
D)  I2 
E)  Ge

Question 8

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains   flask B contains O3,and flask C contains F2.Which flask contains the largest number of molecules?

Accepted Answer

A)  flask A 
B)  flask B 
C)  flask C 
D)  All contain same number of molecules. 
A)  flask A 
B)  flask B 
C)  flask C 
D)  All contain same number of molecules.

Question 9

Given the equation C2H6(g)+ O2(g)→ CO2(g)+ H2O(g)(not balanced),determine the number of liters of CO2 formed at STP when 240.0 grams of C2H6 is burned in excess oxygen gas.

Accepted Answer

Question 10

Determine the volume of SO2 (at STP)formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm).The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s)+ 11 O2(g)→ 2 Fe2O3(s)+ 8 SO2(g)

Accepted Answer

A)  36.1 L 
B)  45.3 L 
C)  18.1 L 
D)  27.6 L 
E)  32.9 L 
A)  36.1 L 
B)  45.3 L 
C)  18.1 L 
D)  27.6 L 
E)  32.9 L

Question 11

Determine the total volume of all gases (at STP)formed when 50.0 mL of TNT (C3H5(NO3)3,d = 1.60 g/mL,molar mass = 227.10 g/mol)reacts according to the following reaction. 4 C3H5(NO3)3(l)→ 6 N2(g)+ O2(g)+ 12 CO2(g)+ 10 H2O(g)

Accepted Answer

A)  4.93 L 
B)  57.2 L 
C)  29.6 L 
D)  448 L 
E)  175 L 
A)  4.93 L 
B)  57.2 L 
C)  29.6 L 
D)  448 L 
E)  175 L

Question 12

A mixture of N2,O2 and He have mole fractions of 0.25,0.65,and 0.10,respectively.What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?

Accepted Answer

A)  2.5 atm 
B)  0.39 atm 
C)  0.67 atm 
D)  0.98 atm 
E)  1.33 atm 
A)  2.5 atm 
B)  0.39 atm 
C)  0.67 atm 
D)  0.98 atm 
E)  1.33 atm

Question 13

Which of the following will cause the volume of an ideal gas to triple in value?

Accepted Answer

A)  raising the temperature from 25°C to 75°C at constant pressure 
B)  lowering the absolute temperature by a factor of 3 at constant pressure 
C)  raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
D)  lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
E)  lowering the pressure by a factor of 3 while the temperature stays constant 
A)  raising the temperature from 25°C to 75°C at constant pressure 
B)  lowering the absolute temperature by a factor of 3 at constant pressure 
C)  raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
D)  lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
E)  lowering the pressure by a factor of 3 while the temperature stays constant

Question 14

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g)and 0.288 mol of N2(g)at 20.0°C?

Accepted Answer

A)  0. 510 atm 
B)  0.681 atm 
C)  1.16 atm 
D)  1.66 atm 
A)  0. 510 atm 
B)  0.681 atm 
C)  1.16 atm 
D)  1.66 atm

Question 15

A sample of N2 effuses in 220 s.How long will the same size sample of Cl2 take to effuse?

Accepted Answer

A)  350 s 
B)  138 s 
C)  558 s 
D)  86.8 s 
E)  388 s 
A)  350 s 
B)  138 s 
C)  558 s 
D)  86.8 s 
E)  388 s

Question 16

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 17

A balloon contains 0.76 mol N2,0.18 mol O2,0.031 mol He and 0.026 mol H2 at 7 49 mm Hg.What is the partial pressure of O2?

Accepted Answer

A)  20 mm Hg 
B)  23 mm Hg 
C)  140 mm Hg 
D)  570 mm Hg 
A)  20 mm Hg 
B)  23 mm Hg 
C)  140 mm Hg 
D)  570 mm Hg

Question 18

A 0.600 g sample containing Ag2O and inert material is heated,causing the silver oxide to decompose according to the following equation: 2 Ag2O(s)→ 4 Ag(s)+ O2(g)
If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure,what is the percentage of silver oxide in the sample?
The partial pressure of water is 26.7 mm Hg at 27°C.

Accepted Answer

A)  10.4% 
B)  20.9% 
C)  41.8% 
D)  44.8% 
A)  10.4% 
B)  20.9% 
C)  41.8% 
D)  44.8%

Question 19

What is the volume of 5.60 g of O2 at 7.78 atm and 415K?

Accepted Answer

A)  1.53 L 
B)  565 L 
C)  24.5 L 
D)  25.0 L 
E)  0.766 L 
A)  1.53 L 
B)  565 L 
C)  24.5 L 
D)  25.0 L 
E)  0.766 L

Question 20

The volume of a gas is proportional to the temperature of a gas is known as

Accepted Answer

A)  Avogadro's Law. 
B)  Ideal Gas Law. 
C)  Charles's Law. 
D)  Boyle's Law. 
E)  Dalton's Law. 
A)  Avogadro's Law. 
B)  Ideal Gas Law. 
C)  Charles's Law. 
D)  Boyle's Law. 
E)  Dalton's Law.

Exam 11: Gases

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl2 at 325 K.What is the partial pressure of Cl2?

A sample of CO2 gas fills a container with a volume of 44.5 L.When the volume is decreased to 13.8 L at a constant temperature,the pressure inside the container is 6.25 atm.What was the pressure inside the container originally?

Which of the following statements is TRUE?

The mole fraction of argon in dry air near sea level is 1.818 × 10-5 where the molar mass of argon is 39.948.The concentration of argon in the atmosphere is ________ ppm.

Why does hot air rise?

The density of chlorine gas at 1.21 atm and 34.9°C is ________ g/L.

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm.What is the identity of the halogen?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains flask B contains O3,and flask C contains F2.Which flask contains the largest number of molecules?

Given the equation C2H6(g)+ O2(g)→ CO2(g)+ H2O(g)(not balanced),determine the number of liters of CO2 formed at STP when 240.0 grams of C2H6 is burned in excess oxygen gas.

Determine the volume of SO2 (at STP)formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm).The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s)+ 11 O2(g)→ 2 Fe2O3(s)+ 8 SO2(g)

Determine the total volume of all gases (at STP)formed when 50.0 mL of TNT (C3H5(NO3)3,d = 1.60 g/mL,molar mass = 227.10 g/mol)reacts according to the following reaction. 4 C3H5(NO3)3(l)→ 6 N2(g)+ O2(g)+ 12 CO2(g)+ 10 H2O(g)

A mixture of N2,O2 and He have mole fractions of 0.25,0.65,and 0.10,respectively.What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?

Which of the following will cause the volume of an ideal gas to triple in value?

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H2(g)and 0.288 mol of N2(g)at 20.0°C?

A sample of N2 effuses in 220 s.How long will the same size sample of Cl2 take to effuse?

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?

A balloon contains 0.76 mol N2,0.18 mol O2,0.031 mol He and 0.026 mol H2 at 7 49 mm Hg.What is the partial pressure of O2?

What is the volume of 5.60 g of O2 at 7.78 atm and 415K?

The volume of a gas is proportional to the temperature of a gas is known as

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A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl₂ at 325 K.What is the partial pressure of Cl₂?

A sample of CO₂ gas fills a container with a volume of 44.5 L.When the volume is decreased to 13.8 L at a constant temperature,the pressure inside the container is 6.25 atm.What was the pressure inside the container originally?

The mole fraction of argon in dry air near sea level is 1.818 × 10^-5 where the molar mass of argon is 39.948.The concentration of argon in the atmosphere is ________ ppm.

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains flask B contains O₃,and flask C contains F₂.Which flask contains the largest number of molecules?

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 240.0 grams of C₂H₆ is burned in excess oxygen gas.

Determine the volume of SO₂ (at STP)formed from the reaction of 96.7 g of FeS₂ and 55.0 L of O₂ (at 398 K and 1.20 atm).The molar mass of FeS₂ is 119.99 g/mol. 4 FeS₂(s)+ 11 O₂(g)→ 2 Fe₂O₃(s)+ 8 SO₂(g)

Determine the total volume of all gases (at STP)formed when 50.0 mL of TNT (C₃H₅(NO₃)₃,d = 1.60 g/mL,molar mass = 227.10 g/mol)reacts according to the following reaction. 4 C₃H₅(NO₃)₃(l)→ 6 N₂(g)+ O₂(g)+ 12 CO₂(g)+ 10 H₂O(g)

A mixture of N₂,O₂ and He have mole fractions of 0.25,0.65,and 0.10,respectively.What is the pressure of N₂ if the total pressure of the mixture is 3.9 atm?

What is the total pressure in a 6.00-L flask which contains 0.127 mol of H₂(g)and 0.288 mol of N₂(g)at 20.0°C?

A sample of N₂ effuses in 220 s.How long will the same size sample of Cl₂ take to effuse?

A balloon contains 0.76 mol N₂,0.18 mol O₂,0.031 mol He and 0.026 mol H₂ at 7 49 mm Hg.What is the partial pressure of O₂?

What is the volume of 5.60 g of O₂ at 7.78 atm and 415K?