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General Chemistry: Gases Properties and Gas Laws

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Terms in this set (20)

  • Kinetic Molecular Theory

    Model explaining gas behavior: particles move constantly and rapidly, collisions are elastic, particles have negligible volume, and speed increases with temperature.

  • Why are gases highly compressible?

    Because of the large empty spaces between particles, gases can be compressed by forcing particles closer together, reducing volume.

  • What causes gas pressure?

    Gas pressure results from collisions of gas particles with the walls of their container.

  • Common units of pressure

    Pascal (Pa), pounds per square inch (psi), torr (mmHg), inches of mercury (in Hg), atmosphere (atm).

  • Blood pressure measurement units

    Measured in millimeters of mercury (mmHg), with systolic and diastolic values indicating different health states.

  • Boyle's Law

    At constant temperature and moles, volume is inversely proportional to pressure: \(P_1V_1 = P_2V_2\).

  • Molecular interpretation of Boyle's Law

    Decreasing volume increases particle collisions with container walls, raising pressure.

  • Charles's Law

    At constant pressure and moles, volume is directly proportional to temperature in Kelvin: \(\frac{V_1}{T_1} = \frac{V_2}{T_2}\).

  • Avogadro's Law

    At constant temperature and pressure, volume is directly proportional to number of moles: \(\frac{V_1}{n_1} = \frac{V_2}{n_2}\).

  • Combined Gas Law

    Relates pressure, volume, and temperature for fixed moles: \(\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}\).

  • Ideal Gas Law

    Combines gas laws: \(PV = nRT\), where R = 0.0821 L·atm/(mol·K).

  • Standard Temperature and Pressure (STP)

    Defined as 0°C and 1 atm; one mole of ideal gas occupies 22.4 L at STP.

  • Density of a gas at STP

    Density (g/L) = Molar mass (g/mol) divided by 22.4 L.

  • Dalton's Law of Partial Pressures

    Total pressure of a gas mixture equals the sum of partial pressures: \(P_{total} = P_1 + P_2 + ... + P_n\).

  • Partial pressure formula

    Partial pressure of component i: \(P_i = X_i \times P_{total}\), where X_i is mole fraction.

  • Relationship between temperature and molecular velocity

    Average kinetic energy and molecular speed increase with temperature; lighter molecules move faster at the same temperature.

  • Diffusion vs Effusion

    Diffusion is gas mixing by molecular motion; effusion is gas escape through a small hole.

  • Graham's Law of Effusion

    Rate ratio of effusion: \(\frac{Rate_1}{Rate_2} = \sqrt{\frac{M_2}{M_1}}\), where M is molar mass.

  • Why do real gases deviate from ideal behavior?

    At high pressure and low temperature, intermolecular attractions and finite particle volume cause deviations.

  • van der Waals equation

    Modified ideal gas law: \(\left(P + a\frac{n^2}{V^2}\right)(V - nb) = nRT\), where a and b correct for attractions and volume.