equilibrium constant kp

• What is the relationship between total pressure and partial pressures?

  Total pressure is the sum of partial pressures
• If the total pressure is 714 kiloPascals and chlorine's partial pressure is 263 kiloPascals, how do you calculate the partial pressure of SO2?

  Subtract chlorine's pressure from total pressure
• Why can't the partial pressure of chlorine be used to determine the pressure of SO2Cl2?

  Because chlorine is a reactant and decreases
• What is the mole fraction of a gas?

  Proportion of a gas in a mixture
• How is the mole fraction of a gas calculated?

  Number of moles of gas divided by total moles
• What is the formula for calculating partial pressure using mole fraction?

  Partial pressure = mole fraction × total pressure
• What does the 'ICE' table stand for in equilibrium calculations?

  Initial, Change, Equilibrium
• How do you calculate the partial pressure of SO2Cl2 in the example?

  Multiply mole fraction by total pressure
• What are the key steps in calculating partial pressures in equilibrium reactions?

  1. Determine total pressure.
  2. Calculate partial pressures using mole fractions.
  3. Use ICE table for changes in moles.
  4. Apply the formula for partial pressure.
• What are the relationships between reactants and products in equilibrium reactions?

  • Reactants decrease in moles.
  • Products increase in moles.
  • Molar ratios must be maintained.
• What is the significance of the ICE table in equilibrium calculations?

  • Organizes initial, change, and equilibrium moles.
  • Helps track changes in moles.
  • Aids in accurate calculations.
• What can be calculated using equilibrium moles?

  Mole fraction and partial pressure
• What is the mole fraction of SO₂Cl₂ if its moles are 1.25?

  0.263
• How is partial pressure calculated?

  Multiply mole fraction by total pressure
• What is the partial pressure if the mole fraction is 0.263 and total pressure is 7.14 kPa?

  188 kPa
• What is the KP equilibrium constant used for?

  Calculating gas equilibrium reactions
• What is the difference between KP and KC?

  KP uses partial pressures, KC uses concentrations
• What is the general form of the KP expression?

  Products' partial pressures over reactants' partial pressures
• How do you calculate KP for the reaction 2A + B ⇌ C + D?

  Use partial pressures in the KP expression
• What happens to KP if the temperature increases and the equilibrium shifts right?

  KP will increase
• What effect does temperature have on KP?

  KP is valid only at one temperature
• How does increasing temperature affect an exothermic reaction's KP?

  KP will decrease
• What does Le Chatelier's principle state about temperature changes?

  The reaction shifts to counteract the change
• What happens to KP if the temperature is decreased in an exothermic reaction?

  KP will increase
• How does pressure affect the value of KP?

  KP is unaffected by pressure changes
• What is the effect of adding a catalyst on KP?

  Catalysts do not affect KP
• What is the role of a catalyst in a reaction?

  It speeds up the rate of reaction
• What are the steps to calculate KP from partial pressures?

  1. Write the KP expression.
  2. Substitute equilibrium partial pressures into the expression.
  3. Calculate the value of KP.
  4. Determine the units by canceling out.
• What factors affect the value of KP?

  • Temperature
  • Pressure
  • Catalysts
• What is the significance of equilibrium constants like KP and KC?

  • Indicate the extent of a reaction
  • Help predict the direction of a reaction
  • Provide insights into reaction dynamics
• How do you determine the units of KP?

  1. Write units for products and reactants.
  2. Cancel out common units.
  3. Invert remaining units if necessary.