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Chemistry Chapter 11 Gases Review
61 Questions
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Chemistry Chapter 11 Gases Review

Created by
@WellBacklitJasmine

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</p> Signup and view all the answers

    Standard temperature and pressure are

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

    Which of the following is not a unit of pressure?

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

    A pressure of 760.0 mm Hg is equal to

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

    A pressure of 20 torr is equal to

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

    Gases collected by water displacement contain

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

    The actual yield of a chemical reaction is generally

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

    Equilibrium is characterized by

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

    Water's relatively high boiling point is the result of

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

    Diffusion is much slower in liquids than in gases because

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

    The bond between oxygen and hydrogen in a water molecule is

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

    The direct relationship between temperature and volume is known as

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

    Absolute zero is equal to

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

    The equivalent value of 273.15 K is

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

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

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

    The combined gas law is expressed by

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

    A pressure of 20 torr is equal to

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

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

    <p>NH3</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</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</p> Signup and view all the answers

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

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

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

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

    The volume of 1 mol of any gas at STP is

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

    Sublimation involves changing from a

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

    Gas molecules will diffuse faster if the

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

    The rate of effusion of a gas does not depend on

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

    Which of these gases diffuses fastest under the same conditions?

    <p>H2</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</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

    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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    Description

    Test your understanding of gas behavior and properties with this flashcard quiz based on Chapter 11 of your chemistry text. Topics covered include the factors influencing gas pressure, the SI unit for pressure, and more. Perfect for exam preparation and review!

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