Chemistry Chapter 11 Gases Review

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Questions and Answers

What causes a gas to exert pressure?

  • Density
  • Temperature
  • Collisions (correct)
  • Elevation

The SI unit for pressure is

  • Newton
  • mm Hg
  • Pascal (correct)
  • Liter

The pressure exerted by a gas does not depend on

  • Temperature
  • Volume
  • The number of moles present
  • The identity of the gas (correct)

At sea level, the average height of mercury in a barometer is

<p>760 mm (A)</p> Signup and view all the answers

Standard temperature and pressure are

<p>0ºC and 1 atm (A)</p> Signup and view all the answers

Which of the following is not a unit of pressure?

<p>newton (B)</p> Signup and view all the answers

A pressure of 760.0 mm Hg is equal to

<p>1.000 atm (D)</p> Signup and view all the answers

A pressure of 20 torr is equal to

<p>20 mm Hg (A)</p> Signup and view all the answers

Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?

<p>Dalton (A)</p> Signup and view all the answers

Gases collected by water displacement contain

<p>H2O(g) (D)</p> Signup and view all the answers

The three states of matter of a particular substance, in order of the strength of intermolecular forces from least to greatest, are

<p>gas, liquid, solid (D)</p> Signup and view all the answers

The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice is called the

<p>unit cell (A)</p> Signup and view all the answers

The actual yield of a chemical reaction is generally

<p>less than the theoretical yield (B)</p> Signup and view all the answers

Equilibrium is characterized by

<p>opposing processes occurring at equal rates (B)</p> Signup and view all the answers

The amount of energy needed to melt one mole of a substance is its molar

<p>enthalpy of fusion (B)</p> Signup and view all the answers

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

<p>an ideal gas (C)</p> Signup and view all the answers

Water's relatively high boiling point is the result of

<p>hydrogen bonding (B)</p> Signup and view all the answers

Diffusion is much slower in liquids than in gases because

<p>liquid particles are closer together (D)</p> Signup and view all the answers

The bond between oxygen and hydrogen in a water molecule is

<p>polar-covalent (B)</p> Signup and view all the answers

For a fixed amount of gas at a constant temperature, the volume increases as the pressure

<p>decreases (D)</p> Signup and view all the answers

The direct relationship between temperature and volume is known as

<p>Charles's law (D)</p> Signup and view all the answers

Raising the temperature of a gas from 0ºC to 273ºC at constant pressure causes the volume to

<p>double (C)</p> Signup and view all the answers

Absolute zero is equal to

<p>-273.15ºC (D)</p> Signup and view all the answers

The equivalent value of 273.15 K is

<p>0ºC (A)</p> Signup and view all the answers

Gay-Lussac's law shows the direct relationship between temperature and

<p>pressure (D)</p> Signup and view all the answers

A graph of pressure versus temperature in kelvins of a gas at constant volume and fixed mass is a(n)

<p>straight line passing through the point (0,0) (B)</p> Signup and view all the answers

The combined gas law is expressed by

<p>(P1V1/T1)=(P2V2/T2) (B)</p> Signup and view all the answers

Assuming all other conditions are constant, what is the new pressure of a gas if the original pressure is 50 kPa and the Kelvin temperature is doubled?

<p>100 kPa (C)</p> Signup and view all the answers

A pressure of 20 torr is equal to

<p>20 mm Hg (B)</p> Signup and view all the answers

The kinetic-molecular theory of gases assumes that the particles of an ideal gas are separated by great distances. This implies that the gas particles are considered to have no definite ______.

<p>volume</p> Signup and view all the answers

If a gas and a liquid are the same temperature and pressure, diffusion occurs much faster in the gas because

<p>the particles move faster in a gas and there is a greater distance between them (D)</p> Signup and view all the answers

If the particles in a sample of matter are attracted to each other but can move past each other easily, the matter is a

<p>liquid (D)</p> Signup and view all the answers

Which gas is most likely to deviate from ideal gas behavior?

<p>NH3 (C)</p> Signup and view all the answers

When there is a small decrease in temperature, the average kinetic energy of the particles of a liquid

<p>decreases (D)</p> Signup and view all the answers

Covalent molecular crystals have very low melting points, while covalent network crystals have very high melting points because

<p>the forces that hold molecules together in molecular crystals are weaker than those that hold molecules or atoms together in network crystals (D)</p> Signup and view all the answers

Water has an unusually high molar enthalpy of vaporization because of its

<p>hydrogen bonding (C)</p> Signup and view all the answers

At the same temperature and pressure, balloons of equal volume always contain

<p>equal numbers of molecules (B)</p> Signup and view all the answers

The person who established that water must contain twice as many hydrogen atoms as oxygen atoms was

<p>Avogadro (D)</p> Signup and view all the answers

The coefficients in a balanced chemical equation involving diatomic gases indicate the relative numbers of all of the following except

<p>atoms (A)</p> Signup and view all the answers

The volume of 1 mol of any gas at STP is

<p>22.41 L (A)</p> Signup and view all the answers

Which law implies that the volume of a gas is directly proportional to the number of moles of the gas?

<p>Avogadro's (A)</p> Signup and view all the answers

The ideal gas law states the relationship among

<p>pressure, volume, temperature, the gas constant, and number of moles (C)</p> Signup and view all the answers

If the pressure and temperature are kept constant, gases react in volume proportions that are

<p>whole numbers (D)</p> Signup and view all the answers

Which is one way of expressing the units for the ideal gas constant?

<p>(L<em>kPa)/(mol</em>K) (B)</p> Signup and view all the answers

In gas stoichiometry problems, the bridge between moles and volume is the ______.

<p>ideal gas law</p> Signup and view all the answers

The value of the gas constant is

<p>0.0821 (L<em>atm)/(mol</em>K) (B)</p> Signup and view all the answers

The ideal gas law combines Boyle's law, Charles's law, Gay-Lussac's law, and __________.

<p>Avogadro's law</p> Signup and view all the answers

Which of the following is true for the melting and freezing points of a pure substance?

<p>The melting point is the same as the freezing point. (C)</p> Signup and view all the answers

Sublimation involves changing from a

<p>solid to a gas (C)</p> Signup and view all the answers

An increase in pressure exerted on a liquid does not compress the liquid as much as the same increase in pressure compresses a gas because

<p>particles are more closely packed in liquids (D)</p> Signup and view all the answers

The process by which the particles of gas randomly pass through a tiny opening is called

<p>effusion (C)</p> Signup and view all the answers

Gas molecules will diffuse faster if the

<p>temperature increases (B)</p> Signup and view all the answers

The gas law that states that the rate of effusion of a gas is inversely proportional to the square root of the molar masses of the gases is

<p>Graham's law (D)</p> Signup and view all the answers

You are measuring the speeds of two particles at the same conditions. The more massive particle will move

<p>at a slower speed (B)</p> Signup and view all the answers

The kinetic energy of the particles in a gas can be expressed as

<p>1/2 mv^2 (A)</p> Signup and view all the answers

The average kinetic energy of the particles in any gas depends only on the

<p>temperature of the gas (C)</p> Signup and view all the answers

The rate of effusion of a gas does not depend on

<p>size of container (D)</p> Signup and view all the answers

Graham's law of effusion is derived from

<p>the equation relating kinetic energy of two different gases under the same conditions (D)</p> Signup and view all the answers

Which of these gases diffuses fastest under the same conditions?

<p>H2 (D)</p> Signup and view all the answers

Under which conditions does a real gas behave very much like an ideal gas?

<p>high temperature and low pressure (B)</p> Signup and view all the answers

The rates of effusion and diffusion depend on the what factor?

<p>velocity</p> Signup and view all the answers

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Study Notes

Gas Pressure and Behavior

  • Gases exert pressure due to collisions between gas particles and the container walls.
  • The SI unit for pressure is the Pascal (Pa).
  • Pressure does not depend on the identity of the gas, but rather on temperature, volume, and the number of moles.

Standard Conditions and Units

  • At sea level, a barometer measures an average mercury height of 760 mm, equating to 1.000 atm.
  • Standard temperature and pressure (STP) are defined as 0ºC and 1 atm.

Gas Relationships and Laws

  • The combined gas law expresses the relationship of pressure, volume, and temperature: (P1V1/T1) = (P2V2/T2).
  • Charles's Law describes the direct relationship between temperature and volume.
  • Gay-Lussac's Law illustrates the direct relationship between temperature and pressure.

Gas Properties

  • The volume of 1 mole of any gas at STP is 22.41 L.
  • The ideal gas law combines various gas laws and relates pressure, volume, temperature, number of moles, and the gas constant.

Diffusion and Effusion

  • Diffusion occurs faster in gases than in liquids due to greater particle separation and motion.
  • Effusion is the process where gas particles escape through a tiny opening; influenced by the rate described by Graham's Law.

Molecular Interactions

  • Water's high boiling point is attributed to hydrogen bonding, a type of strong intermolecular force.
  • The bond in a water molecule between oxygen and hydrogen is characterized as polar-covalent.

Kinetic Molecular Theory

  • Assumes that gas particles are far apart and have negligible volume compared to the total volume occupied by the gas.
  • The average kinetic energy of gas particles depends solely on the gas temperature.

Real and Ideal Gases

  • Real gases deviate from ideal behavior primarily at low temperatures and high pressures, while ideal gases behave reliably under high temperatures and low pressures.

Chemical Reactions and Yield

  • The actual yield in a reaction is often less than the theoretical yield.
  • Equilibrium occurs when opposing processes occur at equal rates, maintaining balance in a closed system.

Particle Behavior

  • Larger gas particles move slower than smaller ones under the same conditions, based on their mass.
  • As temperature increases, gas diffusion rates also increase due to higher particle velocities.

Unit Conversions

  • The conversion from torr to Pa indicates that 1 torr is approximately equal to 133.322 Pa.
  • Understanding gas stoichiometry requires using the ideal gas law as a bridge between moles and volume.

Additional Concepts

  • Sublimation refers to the transition of a substance from a solid to a gas without passing through the liquid state.
  • The three states of matter, ranked by the strength of intermolecular forces, are gas, liquid, and solid (from least to greatest).

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