Question 1

A 25.0 L cylinder contains 2.50 *102 g of CH4. What is the pressure in the cylinder at 27.0°C calculated using van der Waals equation?

Accepted Answer

A)  2850 kPa 
B)  1510 kPa 
C)  3870 kPa 
D)  4870 kPa 
E)  5870 kPa 
A)  2850 kPa 
B)  1510 kPa 
C)  3870 kPa 
D)  4870 kPa 
E)  5870 kPa B

Question 2

Explain Robert Boyle's J-shaped tube experiments that determined the quantitative relationship between the pressure and the volume of a gas.

Accepted Answer

Boyle used a J-shaped tube partially filled with mercury, to determine the relationship between gas pressure and volume. In these experiments, a small amount of a gas or air is trapped above the mercury column, and its volume is measured at atmospheric pressure and constant temperature. More mercury is then poured into the open arm to increase the pressure on the gas sample. The pressure on the gas is atmospheric pressure plus the difference in the heights of the mercury columns, and the resulting volume is measured. This process is repeated until either there is no more room in the open arm or the volume of the gas is too small to be measured accurately. Data such as those from one of Boyle's own experiments may be plotted in several ways. A simple plot of V versus P gives a curve called a hyperbola and reveals an inverse relationship between pressure and volume: as the pressure is doubled, the volume decreases by a factor of two. This relationship between the two quantities is described as follows:
PV = constant
Dividing both sides by P gives an equation illustrating the inverse relationship between P and V:
V$\infty$$\frac { 1 } { P }$ This relationship between pressure and volume is known as Boyle's law.

Question 3

A man weighing 750 kg stands on a stool. If the stool has four legs and each leg equals a surface area of 25 cm2, what is the pressure exerted by the man on the floor?

Accepted Answer

A)  75.0 kPa 
B)  735 kPa 
C)  105 kpa 
D)  1880 Pa 
E)  147 kPa 
A)  75.0 kPa 
B)  735 kPa 
C)  105 kpa 
D)  1880 Pa 
E)  147 kPa B

Question 4

Based on their position in the periodic table, which of the following would be a gas?

Accepted Answer

A)  Potassium 
B)  Ruthenium 
C)  Vanadium 
D)  Hydrogen 
E)  Calcium 
A)  Potassium 
B)  Ruthenium 
C)  Vanadium 
D)  Hydrogen 
E)  Calcium

Question 5

The elements that occur naturally as gases are on the _____ side of the periodic table.

Accepted Answer

The answer of The elements that occur naturally as gases...

Question 6

The partial pressures of oxygen in atmospheric air and in air exhaled by a human are in the ratio of 4:3. If the mole fraction of oxygen in atmospheric air is 0.21, how much oxygen is utilized per liter of air breathed?

Accepted Answer

A)  5.2 mL 
B)  11 mL 
C)  158 mL 
D)  14 mL 
E)  21 mL 
A)  5.2 mL 
B)  11 mL 
C)  158 mL 
D)  14 mL 
E)  21 mL

Question 7

An oxygen cylinder used by scuba divers contains 21% of oxygen (mimicking air). Pure oxygen at a pressure above 1 atmosphere is toxic. If the undersea pressure increases by one atmosphere every 33 feet, how deep can a diver using the oxygen cylinder dive before the oxygen gets toxic?

Accepted Answer

A)  99 ft. 
B)  112 ft 
C)  174.67 ft 
D)  157ft 
E)  225 ft 
A)  99 ft. 
B)  112 ft 
C)  174.67 ft 
D)  157ft 
E)  225 ft

Question 8

At constant temperature and volume, the pressure exerted by a gas depends on only the total number of moles of gas present.

Accepted Answer

A) True 
 B)False

Question 9

At what temperature will the volume of a gas be equal to zero?

Accepted Answer

A)  0˚C 
B)  -273.15 K 
C)  273.15 K 
D)  0 K 
E)  273.15˚C 
A)  0˚C 
B)  -273.15 K 
C)  273.15 K 
D)  0 K 
E)  273.15˚C

Question 10

The root mean squared speed of a gas particle increases as the temperature of the gas _____.

Accepted Answer

The answer of The root mean squared speed of a...

Question 11

The value of the universal gas constant in terms of J/K.mol is 0.082057.

Accepted Answer

A) True 
 B)False

Question 12

A 10.0 L cylinder contains 370.0 g of N2. Its pressure to three significant figures at 27.0 °C calculated using van der Waals equation is _____.

Accepted Answer

A)  31.9 atm 
B)  9.50 atm 
C)  325 atm 
D)  2.36 atm 
E)  456 atm 
A)  31.9 atm 
B)  9.50 atm 
C)  325 atm 
D)  2.36 atm 
E)  456 atm

Question 13

As the density of a gas decreases, the mean free path becomes _____.

Accepted Answer

The answer of As the density of a gas decreases,...

Question 14

In a gas, attractive intermolecular forces produce a pressure that is more than that expected based on the ideal gas law.

Accepted Answer

A) True 
 B)False

Question 15

A 25.0 L cylinder contains 2.50 *102 g of CH4. What is the difference in the pressure at 27.0°C calculated using van der Waals equation, and the pressure calculated using the ideal gas equation?

Accepted Answer

A)  0 kPa 
B)  105 kPa 
C)  20.4 kPa 
D)  77.6 kPa 
E)  46.6 kPa 
A)  0 kPa 
B)  105 kPa 
C)  20.4 kPa 
D)  77.6 kPa 
E)  46.6 kPa

Question 16

The speed of 8 particles were found to be 2, 2, 4, 5, 5, 7, 6, and 6 m/s, the root mean squared speed of the particles are _____ m/s.

Accepted Answer

A)  5.000 
B)  4.937 
C)  24.37 
D)  37.00 
E)  1.348 
A)  5.000 
B)  4.937 
C)  24.37 
D)  37.00 
E)  1.348

Question 17

The partial pressure of a gas is independent of the pressure exerted by all other gases present.

Accepted Answer

A) True 
 B)False

Question 18

The volume of a container containing a gas is increased by 50%. Which of the following quantities decreases?

Accepted Answer

A)  Average velocity of the gas particles 
B)  Root mean squared speed of the gas particles 
C)  Average speed of the gas particles 
D)  Force exerted by the gas per unit area of the container 
E)  The number of gas particle within the container 
A)  Average velocity of the gas particles 
B)  Root mean squared speed of the gas particles 
C)  Average speed of the gas particles 
D)  Force exerted by the gas per unit area of the container 
E)  The number of gas particle within the container

Question 19

Which of the following is not a gas at room temperature?

Accepted Answer

A)  Hydrogen 
B)  Fluorine 
C)  Bromine 
D)  Iodine 
E)  Mercury 
A)  Hydrogen 
B)  Fluorine 
C)  Bromine 
D)  Iodine 
E)  Mercury

Question 20

One mole of a gas at 25˚C at a pressure of 2 atms has a volume of 17.8 L. What will the volume of the gas be at a temperature of 35˚C?

Accepted Answer

A)  16.4 L 
B)  12.7 L 
C)  17.8 L 
D)  18.4 L 
E)  22.4 L 
A)  16.4 L 
B)  12.7 L 
C)  17.8 L 
D)  18.4 L 
E)  22.4 L

Exam 10: Gases

A 25.0 L cylinder contains 2.50 *102 g of CH4. What is the pressure in the cylinder at 27.0°C calculated using van der Waals equation?

Explain Robert Boyle's J-shaped tube experiments that determined the quantitative relationship between the pressure and the volume of a gas.

A man weighing 750 kg stands on a stool. If the stool has four legs and each leg equals a surface area of 25 cm2, what is the pressure exerted by the man on the floor?

Based on their position in the periodic table, which of the following would be a gas?

The elements that occur naturally as gases are on the _____ side of the periodic table.

The partial pressures of oxygen in atmospheric air and in air exhaled by a human are in the ratio of 4:3. If the mole fraction of oxygen in atmospheric air is 0.21, how much oxygen is utilized per liter of air breathed?

An oxygen cylinder used by scuba divers contains 21% of oxygen (mimicking air). Pure oxygen at a pressure above 1 atmosphere is toxic. If the undersea pressure increases by one atmosphere every 33 feet, how deep can a diver using the oxygen cylinder dive before the oxygen gets toxic?

At constant temperature and volume, the pressure exerted by a gas depends on only the total number of moles of gas present.

At what temperature will the volume of a gas be equal to zero?

The root mean squared speed of a gas particle increases as the temperature of the gas _____.

The value of the universal gas constant in terms of J/K.mol is 0.082057.

A 10.0 L cylinder contains 370.0 g of N2. Its pressure to three significant figures at 27.0 °C calculated using van der Waals equation is _____.

As the density of a gas decreases, the mean free path becomes _____.

In a gas, attractive intermolecular forces produce a pressure that is more than that expected based on the ideal gas law.

A 25.0 L cylinder contains 2.50 *102 g of CH4. What is the difference in the pressure at 27.0°C calculated using van der Waals equation, and the pressure calculated using the ideal gas equation?

The speed of 8 particles were found to be 2, 2, 4, 5, 5, 7, 6, and 6 m/s, the root mean squared speed of the particles are _____ m/s.

The partial pressure of a gas is independent of the pressure exerted by all other gases present.

The volume of a container containing a gas is increased by 50%. Which of the following quantities decreases?

Which of the following is not a gas at room temperature?

One mole of a gas at 25˚C at a pressure of 2 atms has a volume of 17.8 L. What will the volume of the gas be at a temperature of 35˚C?

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Liquids

Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Acidbase Equilibriums

Solubility and Complexation Equilibriums

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Periodic Trends and the S-Block Elements

The P-Block Elements

The D-Block Elements

Organic Compounds

Filters

A 25.0 L cylinder contains 2.50 *10² g of CH₄. What is the pressure in the cylinder at 27.0°C calculated using van der Waals equation?

A man weighing 750 kg stands on a stool. If the stool has four legs and each leg equals a surface area of 25 cm², what is the pressure exerted by the man on the floor?

A 10.0 L cylinder contains 370.0 g of N₂. Its pressure to three significant figures at 27.0 °C calculated using van der Waals equation is _____.

A 25.0 L cylinder contains 2.50 *10² g of CH₄. What is the difference in the pressure at 27.0°C calculated using van der Waals equation, and the pressure calculated using the ideal gas equation?