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CHM 211; CH.5: Gas Laws and Molecular Nature of Matter

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Terms in this set (20)

  • What is atmospheric pressure at sea level in common units?
    1 atm = 760 mmHg = 101.325 kPa
  • What are the standard temperature and pressure (STP) conditions?
    1 atm pressure and 0 °C (273 K) temperature
  • How do gases differ from liquids and solids in terms of volume change?
    Gas volume changes significantly with pressure and temperature, unlike solids and liquids.
  • State Boyle's Law and its formula.
    At constant temperature, volume is inversely proportional to pressure: \(PV=\text{constant}\) or \(P_1V_1=P_2V_2\)
  • State Charles's Law and its formula.
    At constant pressure, volume is directly proportional to absolute temperature: \(\frac{V}{T}=\text{constant}\) or \(\frac{V_1}{T_1}=\frac{V_2}{T_2}\)
  • State Avogadro's Law and its formula.
    At constant temperature and pressure, volume is directly proportional to moles: \(\frac{V}{n}=\text{constant}\) or \(\frac{V_1}{n_1}=\frac{V_2}{n_2}\)
  • What is the Ideal Gas Law formula?
    \(PV=nRT\), relating pressure, volume, moles, and temperature.
  • What are the ideal gas assumptions?
    No intermolecular forces, gas molecules have negligible volume, and collisions are elastic with no kinetic energy loss.
  • What volume does 1 mole of an ideal gas occupy at STP?
    22.4 L at 0 °C and 1 atm
  • How do you calculate the density of a gas using the ideal gas law?
    \(d=\frac{MP}{RT}\), where M is molar mass.
  • What is Dalton's Law of Partial Pressures?
    Total pressure is the sum of partial pressures: \(P_T=P_A+P_B+\cdots\) and \(P_A=X_AP_T\) where X_A is mole fraction.
  • What does the kinetic molecular theory state about gas molecules?
    Gas molecules are in constant, random motion with a distribution of speeds related to temperature.
  • How is the average kinetic energy of gas molecules related to temperature?
    \(KE=\frac{3}{2}k_BT\), where k_B is Boltzmann's constant.
  • What is the formula for root-mean-square speed of gas molecules?
    \(u_{rms}=\sqrt{\frac{3RT}{M}}\), where M is molar mass in kg/mol.
  • State Graham's Law of Effusion and Diffusion.
    Rate ratio relates inversely to square root of molar masses: \(\frac{r_1}{r_2}=\sqrt{\frac{M_2}{M_1}}\)
  • Why do real gases deviate from ideal gas behavior?
    Real gases have finite volume and experience intermolecular forces, especially at low temperature and high pressure.
  • What is the Van der Waals equation for real gases?
    \(\left(P+\frac{n^2a}{V^2}\right)(V-nb)=nRT\), where a and b correct for attractions and volume.
  • How does gas volume change with temperature at constant pressure?
    Gas volume increases as temperature increases, according to Charles's Law.
  • How does gas pressure change with volume at constant temperature?
    Gas pressure increases as volume decreases, according to Boyle's Law.
  • How do you calculate molar mass from the ideal gas law?
    \(M=\frac{mRT}{PV}\), where m is mass of gas.