Chemistry Chapter 11 - Gases
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Questions and Answers

Which statement best describes an ideal gas according to the Kinetic Molecular Theory?

  • It has significant forces of attraction between particles.
  • It has a definite volume and attracts other gases.
  • It experiences elastic collisions and has no volume. (correct)
  • It compresses easily and has high density.

    • Real gases behave ideally at low temperatures and high pressures.

    False

    What is the universal gas constant in liter·atm/(K·mol)?

    0.0821

    According to Boyle's Law, when the volume of a gas increases, its _____ decreases.

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

    Match each term with the correct description:

    <p>Avogadro's Principle = Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules Ideal Gas Law = PV=nRT Gas Stoichiometry = Deals with the relationships between volumes of gases and moles in reactions Universal Gas Constant = The constant R in the ideal gas law equations</p> Signup and view all the answers

    Which of the following scenarios illustrates gas diffusion?

    <p>Perfume scent spreading in a room.</p> Signup and view all the answers

    At STP, the temperature of a gas is measured in Celsius.

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

    What effect does increasing temperature have on the average kinetic energy of gas particles?

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

    According to Charles' Law, what happens to the volume of a gas when the temperature increases, assuming constant mass and pressure?

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

    Gay-Lussac's Law states that the pressure and volume of a gas are directly related.

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

    What is the relationship described by the Combined Gas Law?

    <p>The relationship among pressure, volume, and temperature of a gas.</p> Signup and view all the answers

    According to Gay-Lussac's Law, P/T = _____ (where k is a constant).

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

    Match the gas law with its application:

    <p>Charles' Law = Volume and temperature relationship at constant pressure Gay-Lussac's Law = Pressure and temperature relationship at constant volume Boyle's Law = Pressure and volume relationship at constant temperature Combined Gas Law = Relationship of pressure, volume, and temperature when all are changing</p> Signup and view all the answers

    What is the value of the universal gas constant (R) in the Ideal Gas Law?

    <p>Both A and B are correct</p> Signup and view all the answers

    Avogadro's Principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

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

    What happens to the volume of a gas when pressure is increased, according to Boyle's Law?

    <p>The volume decreases.</p> Signup and view all the answers

    What is the ideal gas constant R in the ideal gas law PV = nRT?

    <p>8.315 dm³·kPa/mol·K</p> Signup and view all the answers

    Dalton's Law states that the total pressure of a mixture of gases is equal to the product of the individual gas pressures.

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

    What volume of CO2 is produced from 5.25 g of CaCO3 at 103 kPa and 25ºC?

    <p>1.26 dm³</p> Signup and view all the answers

    The temperature must be converted to ______ for gas law calculations.

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

    Match the gas parameters to their corresponding values in the first problem:

    <p>Pressure (P) = 103 kPa Temperature (T) = 25°C Number of moles (n) = 0.052 mol Volume (V) = 1.26 dm³</p> Signup and view all the answers

    How many grams of Al2O3 are formed from 15.0 L of O2 at 97.3 kPa and 21°C?

    <p>40.6 g</p> Signup and view all the answers

    To find the partial pressure of a gas, you subtract the water vapor pressure from the total pressure.

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

    What is the partial pressure of dry hydrogen gas if the atmospheric pressure is 94.4 kPa and the water vapor pressure is 2.72 kPa?

    <p>91.7 kPa</p> Signup and view all the answers

    Study Notes

    Chapter 11 - Gases

    • Gases expand to fill any container.
    • Gases are fluids (like liquids).
    • Gases have very low densities.
    • Gases can be compressed.
    • Gases undergo diffusion and effusion.

    I. Physical Properties (of gases)

    • Kinetic Molecular Theory (ideal gas):

      • Particles have no volume.
      • Particles have elastic collisions.
      • Particles are in constant, random, straight-line motion.
      • Particles do not attract or repel each other.
      • Average kinetic energy is directly related to Kelvin temperature.

    • Real Gases:

      • Particles have their own volume.
      • Particles attract each other.
      • Gas behavior is most ideal:
        • At low pressure.
        • At high temperatures.
        • Nonpolar atoms/molecules.

    II. Temperature

    • Always use absolute temperature (Kelvin) when working with gases.
    • °C = 5/9 (°F - 32)
    • K = °C + 273

    III. Pressure

    • Pressure = force/area
    • Which shoes create the most pressure? (This question relates to the concept of pressure on different areas, not the actual shoes.)
    • Barometer: Measures atmospheric pressure
      • Mercury Barometer
      • Aneroid Barometer
    • Key Units at Sea Level:
      • 101.325 kPa (kilopascal)
      • 1 atm
      • 760 mm Hg
      • 760 torr
      • 14.7 psi

    IV. STP (Standard Temperature & Pressure)

    • 0°C or 273 K
    • 1 atm or 101.325 kPa

    V. Gas Laws

    • Boyle's Law:

      • Pressure and volume are inversely related (at constant mass and temperature)
      • PV = k

    • Charles' Law:

      • Volume and absolute temperature are directly related (at constant mass and pressure)
      • V/T = k

    • Gay-Lussac's Law:

      • Pressure and absolute temperature are directly related (at constant mass and volume)
      • P/T = k

    • Combined Gas Law:

      • P₁V₁/T₁ = P₂V₂/T₂ (or P₁V₁T₂ = P₂V₂T₁)

    VI. Ideal Gas Law

    • PV = nRT

    • R=0.0821 L⋅atm/mol⋅K or 8.315 dm³⋅kPa/mol⋅K (Universal Gas Constant)

    • Note: n = moles, P = pressure, V = volume, T = temperature, and R = the Ideal Gas Law constant

    VII. Gas Stoichiometry

    • Moles to Liters of a Gas
      • STP: Use 22.4 L/mol.
      • Non-STP: Use the Ideal Gas Law.
    • Non-STP Problems
      • Given liters of gas: Start with Ideal Gas Law.
      • Looking for liters of gas: Start with stoichiometry conversion.

    VIII. Dalton's Law

    • The total pressure of a mixture of gases equals the sum of the partial pressures of the individual gases.
    • Ptotal = P1 + P2 + ...

    IX. Graham's Law

    • Diffusion: Spreading of gas molecules until evenly distributed.
    • Effusion: Passing of gas molecules through a tiny opening.
    • Speed of diffusion/effusion
      • Kinetic energy is determined by the temperature of the gas.
      • At the same temp & KE, heavier molecules move more slowly.
      • Rate of diffusion is inversely related to the square root of its molar mass

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    Description

    Explore the fascinating properties of gases in this quiz based on Chapter 11. Learn about the Kinetic Molecular Theory, the behavior of real gases, and the relationship between temperature and pressure. Test your knowledge on key concepts and definitions related to gases.

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