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Chem Ch6

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Termini in questo insieme (21)

  • What is gas pressure?

    Gas pressure is the force exerted per unit area by gas molecules as they collide with surfaces around them.

  • How does altitude affect atmospheric pressure?

    Atmospheric pressure decreases with increasing altitude because the number of gas particles in a given volume decreases.

  • What factors affect gas pressure?

    Gas pressure depends on the number of gas particles, the volume of the container, and the average speed of the gas particles.

  • State Boyle's Law.

    At constant temperature and amount, the pressure of a gas is inversely proportional to its volume: \(P \times V = \text{constant}\).

  • Explain the molecular interpretation of Boyle's Law.

    Decreasing the volume increases the frequency of molecular collisions with container walls, increasing pressure.

  • What is Charles's Law?

    At constant pressure and amount, the volume of a gas is directly proportional to its temperature in kelvins: \(\frac{V}{T} = \text{constant}\).

  • What is absolute zero in terms of Charles's Law?

    Absolute zero is the temperature at which the volume of a gas extrapolates to zero, 0 K or -273.15 °C.

  • State Avogadro's Law.

    At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles: \(\frac{V}{n} = \text{constant}\).

  • What is the Ideal Gas Law?

    The combined gas law: \(PV = nRT\), relating pressure, volume, temperature, and moles.

  • What are the standard temperature and pressure (STP) conditions?

    Standard temperature is 273 K (0 °C) and standard pressure is 1 atm.

  • What is the molar volume of an ideal gas at STP?

    One mole of an ideal gas occupies 22.4 liters at STP.

  • How is gas density related to molar mass at STP?

    Density = molar mass / molar volume; gases with higher molar mass have higher density.

  • What is Dalton's Law of Partial Pressures?

    The total pressure of a gas mixture equals the sum of the partial pressures of each component: \(P_{total} = P_a + P_b + P_c + \cdots\).

  • How is mole fraction defined in gas mixtures?

    Mole fraction is the ratio of moles of a component to total moles: \(\chi_a = \frac{n_a}{n_{total}}\).

  • What is the relationship between partial pressure and mole fraction?

    Partial pressure of a gas = mole fraction × total pressure: \(P_a = \chi_a P_{total}\).

  • What is the kinetic molecular theory assumption about gas particles?

    Gas particles are in constant motion, have negligible size, no intermolecular attractions, and collisions are elastic.

  • How does temperature affect the average kinetic energy of gas particles?

    Average kinetic energy is directly proportional to temperature in kelvins.

  • What is the root mean square velocity formula for gas molecules?

    \(u_{rms} = \sqrt{\frac{3RT}{M}}\), where M is molar mass in kg/mol.

  • What is Graham's Law of Effusion?

    The rate of effusion of a gas is inversely proportional to the square root of its molar mass: \(\frac{rate_A}{rate_B} = \sqrt{\frac{M_B}{M_A}}\).

  • Why do real gases deviate from ideal gas behavior?

    Real gases have intermolecular attractions and finite molecular volume, especially at high pressure and low temperature.

  • What is the van der Waals equation?

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