Equilibrium Constant KpFlashcards - AQA Chemistry

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Equilibrium Constant Kp

A-Level AQA Chemistry

This pack of flashcards covers the principles of gas mixtures and chemical equilibrium, focusing on concepts such as partial pressure, mole fraction, calculating Kp, and the effects of temperature and pressure on equilibrium. It includes definitions, calculations, and relationships pertinent to gaseous reactions and equilibrium constants.

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"Define Kp in terms of pressure and mole fraction."	"Kp = (N2.P)(X3H2.P3)/(P4), where P is total pressure and X is mole fraction."
"How does increasing pressure affect the position of equilibrium in a reaction with more moles of gas on the product side?"	"Increasing pressure will shift the equilibrium to the right, increasing the mole fractions of products and decreasing the mole fractions of reactants."
"Explain the effect of pressure on the position of equilibrium and Kp in a reaction with fewer moles of gas on the product side."	"Increasing pressure will shift the equilibrium to the side with fewer moles of gas, and the value of Kp stays the same."
"What happens to the equilibrium position and Kp when the temperature is increased in an exothermic reaction?"	"The equilibrium shifts left, and the value of Kp gets smaller as there are fewer products."
"Describe the effect of changing conditions on the value of K or Kp."	"K and Kp only change with temperature. They do not change if pressure or concentration are altered. A catalyst also has no effect on K or Kp."
"Define mole fractions."	"Mole fractions are the ratio of moles of a component to the total moles in a mixture."
"Describe what partial pressure is in a gas mixture."	"Partial pressure is the pressure that a gas would have if it alone occupied the volume occupied by the whole mixture."
"Describe the relationship between total pressure and partial pressures in a gas mixture."	"In a gas mixture, the total pressure is equal to the sum of the partial pressures of all the gases present."
"How would you calculate the mole fraction of N2 in the given mixture?"	"To calculate the mole fraction of N2, divide the number of moles of N2 by the total number of moles of all gases in the mixture."
"Define the equilibrium constant, Kp."	"Kp is the equilibrium constant that relates the partial pressures of the reactants and products in a gaseous reaction at a specific temperature."
"Do solids, liquids, and aqueous substances contribute to the equilibrium constant expression, Kp?"	"No, only gases are included in the Kp expression. Solids, liquids, and aqueous substances are ignored."
"How do you calculate the partial pressure of a gas in a mixture?"	"To calculate the partial pressure of a gas, multiply its mole fraction by the total pressure of the mixture."
"Define mole fraction in the context of gas mixtures."	"Mole fraction is the ratio of the number of moles of a specific gas to the total number of moles of all gases in a mixture."

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