CHM 201

• What are the three physical states of matter?

  Solids, liquids, and gases
• What is H2O known as in its solid state?

  Ice
• What are liquids and gases collectively referred to as?

  Fluids
• Why are solids and liquids referred to as condensed states?

  Because they have much higher densities than gases
• What are the major gaseous components of the Earth's atmosphere?

  N2 and O2
• What does it mean for gases to be miscible?

  They mix completely unless they react with one another
• What happens to gas volume when pressure is increased?

  The volume decreases
• How do gases behave in terms of occupying space?

  They expand without limits to occupy the volume of any container
• What is the relationship between temperature and gas volume at constant pressure?

  Gas volume increases with temperature
• What is Boyle's Law?

  At a given temperature, the product of pressure and volume of a definite mass of gas is constant

  
• What does the equation \(PV = k\) represent in Boyle's Law?

  The product of pressure and volume is constant for a given mass of gas

  
• What happens to gas volume when pressure is applied at constant temperature?

  The volume is inversely proportional to the applied pressure
• What is Charles's Law?

  At constant pressure, the volume occupied by a definite mass of a gas is directly proportional to its absolute temperature

  
• How is temperature expressed in Charles's Law?

  In absolute (Kelvin) scale
• What is the Combined Gas Law Equation?

  \( \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \)

  
• What does Avogadro's Law state?

  At the same temperature and pressure, equal volumes of all gases contain the same number of molecules
• What is the ideal gas equation?

  \( PV = nRT \)

  
• What is the value of the gas constant \( R \) in J/mol·K?

  1. 314 J/mol·K
• What does Dalton's Law of Partial Pressures state?

  The total pressure exerted by a mixture of ideal gases is the sum of the partial pressures of those gases

  
• How is the mole fraction of a component in a gas mixture defined?

  As the ratio of the number of moles of that component to the total number of moles in the mixture

  
• What is the basic assumption of the kinetic-molecular theory regarding gas molecules?

  Gases consist of discrete molecules that are very small and far apart
• What does the average kinetic energy of gaseous molecules relate to?

  It is directly proportional to the absolute temperature of the sample

  
• Under what conditions do real gases deviate from ideal behavior?

  At high pressures and/or low temperatures
• What correction factor is used for real gases in the kinetic-molecular theory?

  The factor \( nb \) corrects for the volume occupied by the molecules themselves
• How does the volume of gas molecules affect the behavior of real gases under high pressure?

  The volume of the molecules becomes a significant fraction of the total volume occupied by the gas
• What happens to the available volume for gas molecules under high pressure?

  The available volume for any molecule to move in is less than the measured volume
• What is the significance of the universal gas constant \( R \) in the ideal gas law?

  It relates the pressure, volume, and temperature of an ideal gas

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

  22.414 liters per mole

  
• How do you calculate the density of a gas at STP?

  By using the formula \( \text{density} = \frac{\text{mass}}{\text{volume}} \)

  
• What is the relationship between the average kinetic energy of gas molecules and their velocities?

  Lighter molecules have higher average velocities than heavier molecules at the same temperature

  
• How does the kinetic-molecular theory explain the behavior of gases under different conditions?

  It relates the properties of gases to their molecular motion and interactions
• Under what conditions is the behavior of gases most significant?

  High pressures and/or low temperatures
• What does the kinetic-molecular theory state about gas molecules?

  Molecules are so small relative to the total volume that they can move through the entire measured volume.
• How does high pressure affect the volume available for gas molecules to move in?

  The available volume for any molecule is less than the measured volume due to the volume occupied by other molecules.
• What is the correction factor used to account for the volume occupied by gas molecules?

  nb
• What does a larger value of b indicate in the context of gas molecules?

  Larger molecules have greater values of b, indicating they occupy more volume.

  
• What happens to the correction term when the volume is large?

  The correction term becomes negligibly small.
• How does the kinetic-molecular theory describe pressure?

  Pressure results from molecular collisions with the walls of the container.
• What effect do intermolecular attractions have on gas pressure at low temperatures?

  At low temperatures, intermolecular attractions become significant, causing fewer collisions and lower pressure.
• What is the correction factor for pressure in the context of real gases?

  We subtract a correction factor, $\frac{n^2a}{V^2}$, from the ideal pressure.