Equilibrium constant Kp

• What is the definition of partial pressure in a gas mixture?

  The partial pressure of a gas is the pressure it would exert if it occupied the entire volume alone.
• How do you calculate the total pressure of a mixture of gases?

  The total pressure equals the sum of the partial pressures of all gases in the mixture.
• What is the formula for calculating the partial pressure of a gas?

  Partial pressure = mole fraction x total pressure.
• How is the mole fraction of a gas defined?

  Mole fraction = number of moles of a gas / total number of moles of all gases.
• What does Kp represent in a chemical reaction?

  Kp is the equilibrium constant for reactions involving gases.
• What should be included in the Kp expression?

  Only gases should be included; solids, liquids, and aqueous substances are ignored.
• How do you calculate the unit of Kp?

  The unit of Kp is \( kPa^{-2} \).
• What happens to Kp if the reaction is reversed?

  The value of Kp will be the inverse of the original Kp value.
• What does a larger Kp value indicate about the equilibrium position?

  A larger Kp indicates a greater amount of products at equilibrium.
• How do Kc and Kp change with temperature?

  Kc and Kp only change with temperature, not with pressure or concentration changes.
• What happens to the equilibrium position if the temperature is increased in an exothermic reaction?

  The equilibrium shifts to the left, favoring the reactants.
• How does increasing pressure affect the equilibrium position in a reaction with fewer moles of gas on the product side?

  The equilibrium shifts to the right, favoring the products.
• What is the relationship between Kp and the mole fractions in the equilibrium expression?

  Kp is calculated using the mole fractions of the gases in the equilibrium expression.
• What are the effects of changing temperature on Kp and the position of equilibrium?

  • Increasing temperature shifts equilibrium in endothermic direction.
  • Decreasing temperature shifts equilibrium in exothermic direction.
  • Kp changes with temperature.
• What are the effects of changing pressure on Kp and the position of equilibrium?

  • Increasing pressure shifts equilibrium towards side with fewer moles of gas.
  • Kp remains constant regardless of pressure changes.