What is the equilibrium constant (Kp) and how is it calculated?
Ch 13 Review

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Chemistry
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11th - 12th Grade
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Hard
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1.
FLASHCARD QUESTION
Front
Back
Kp is a measure of the ratio of the concentrations of products to reactants at equilibrium for a gas-phase reaction, expressed in terms of partial pressures. It is calculated using the formula Kp = (P_products^coefficients)/(P_reactants^coefficients).
2.
FLASHCARD QUESTION
Front
What happens to the equilibrium position when the pressure of a system is increased?
Back
Increasing the pressure of a system at equilibrium will shift the equilibrium position towards the side with fewer moles of gas.
3.
FLASHCARD QUESTION
Front
How do you determine the effect of volume changes on equilibrium?
Back
Decreasing the volume of a gas system increases pressure, favoring the side with fewer moles of gas. Increasing the volume decreases pressure, favoring the side with more moles of gas.
4.
FLASHCARD QUESTION
Front
What is the relationship between Kp and Kc?
Back
Kp and Kc are related by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas (moles of products - moles of reactants).
5.
FLASHCARD QUESTION
Front
How do you calculate the equilibrium constant (K) from concentrations?
Back
K is calculated using the formula K = [products]^coefficients / [reactants]^coefficients at equilibrium.
6.
FLASHCARD QUESTION
Front
What is the significance of a large K value?
Back
A large K value (>>1) indicates that at equilibrium, the reaction favors the formation of products.
7.
FLASHCARD QUESTION
Front
What does a small K value indicate about a reaction?
Back
A small K value (<<1) indicates that at equilibrium, the reaction favors the formation of reactants.
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