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• What is the definition of a gas?

  A gas is a phase of matter where atoms are in motion and fill their container.
• What are the two simplifying assumptions made about ideal gases?

  Particles are dimensionless points in random motion and do not interact except for elastic collisions.
• Why are ideal gases considered useful despite not being completely true?

  They simplify calculations and provide surprisingly accurate predictions.
• What are the four variables discussed when examining an ideal gas?

  • Pressure
  • Temperature
  • Volume
  • Moles
• How does pressure relate to the motion of gas particles?

  Pressure is the force exerted by gas particles hitting the sides of their container.
• What happens to gas particles when the temperature increases?

  The particles move faster as more heat energy is converted into kinetic energy.
• What is Boyle's Law?

  Boyle's Law states that pressure and volume are inversely proportional: \( P_1V_1 = P_2V_2 \).
• If the volume of a gas is halved, what happens to its pressure according to Boyle's Law?

  The pressure doubles.
• What is Charles's Law?

  Charles's Law states that volume and temperature are directly proportional when pressure is constant.
• What happens to the volume of a gas in a balloon when it is heated?

  The volume expands to maintain constant pressure.
• What temperature scale must be used in gas calculations?

  The Kelvin scale must be used.
• Why do we use the Kelvin scale in gas calculations?

  To avoid mathematical issues with negative or zero temperatures.
• How do you convert Celsius to Kelvin?

  Add 273 to the Celsius temperature.
• What is Avogadro's Law?

  Avogadro's Law states that equal volumes of gas at the same temperature and pressure contain the same number of molecules.
• How many liters does one mole of an ideal gas occupy at standard temperature and pressure?

  22.4 liters.
• What is the Ideal Gas Law equation?

  The Ideal Gas Law is expressed as \( PV = nRT \).
• How can you use the Ideal Gas Law if you know three of the four variables?

  You can solve for the fourth variable using the equation \( PV = nRT \).
• What should you do if you have initial and final conditions of a gas?

  You can use Boyle's Law or Charles's Law to find the other information.
• What are the relationships between the variables of an ideal gas?

  • Pressure and Volume: Inversely proportional (Boyle's Law)
  • Volume and Temperature: Directly proportional (Charles's Law)
  • Moles and Volume: Directly proportional (Avogadro's Law)
• What is the gas constant \( R \) used for in the Ideal Gas Law?

  It makes calculations intelligible in manmade units.
• How can the Ideal Gas Law be useful in practical scenarios?

  It allows for quick calculations of gas properties when three variables are known.
• How do Boyle's Law and Charles's Law relate to the Ideal Gas Law?

  They are specific cases of the Ideal Gas Law that describe relationships between two variables while holding others constant.
• What is the relationship between the velocities of molecules and temperature?

  As temperature increases, the average velocity of molecules increases.
• What happens to the distribution of molecular speeds when the temperature is increased?

  The distribution of molecular speeds becomes broader, with some molecules moving faster and some moving slower.
• What is the Maxwell-Boltzmann velocity distribution?

  • Describes the distribution of speeds of particles in a gas
  • Based on the kinetic theory of gases
  • Influenced by temperature and pressure
• At what temperature does the maximum density of molecules occur in the given example?

  The maximum density of molecules occurs at 300 Kelvin.
• How does increasing the temperature to 700 Kelvin affect molecular speeds compared to 500 Kelvin?

  Molecular speeds increase on average at 700 Kelvin compared to 500 Kelvin.
• What is the formula for the kinetic energy of a molecule?

  The kinetic energy \( E_{kin} \) of a molecule is given by \( E_{kin} = \frac{1}{2} m v^2 \).
• Why are not all molecules at zero kinetic energy at a given temperature?

  Because temperature influences the distribution of molecular speeds, resulting in varying kinetic energies.
• What factors influence the velocities of molecules in a gas?

  • Temperature: Higher temperatures lead to higher average velocities
  • Kinetic energy: Related to mass and velocity of molecules
  • Distribution of speeds: Varies with temperature and pressure