AP Chemistry equilibrium ICE key terms
Study key terms and concepts related to equilibrium in AP Chemistry using ICE (Initial, Change, Equilibrium) tables and related terminology.
Quiz(13 pytania)
1. What does an equilibrium constant K > 1 indicate?
Pojęcia w tym zestawie(17)
What does ICE stand for?
ICE stands for Initial, Change, and Equilibrium concentrations.
Define equilibrium in chemistry.
Equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
True or false: Equilibrium is static.
False, because equilibrium is dynamic; reactions continue at equal rates.
Difference between Kc and Kp.
Kc is based on molarity, while Kp is based on partial pressures.
What is the equilibrium constant expression?
For aA + bB ⇌ cC + dD, K = \\frac{[C]^c[D]^d}{[A]^a[B]^b}.
Fill in the blank: At equilibrium, the __________ concentrations remain constant.
reactant and product
What shifts equilibrium to the right?
Adding reactants or removing products shifts equilibrium to the right.
What effect does increasing temperature have on an endothermic reaction?
It shifts the equilibrium to the right, favoring product formation.
Define Le Chatelier's principle.
Le Chatelier's principle states that a system at equilibrium will shift to counteract changes.
True or false: Catalysts affect equilibrium position.
False, because catalysts only speed up the rate of reaching equilibrium.
What does a large K value indicate?
A large K value indicates that at equilibrium, products are favored over reactants.
Difference between Q and K.
Q is the reaction quotient, while K is the equilibrium constant at a specific temperature.
Fill in the blank: A decrease in volume shifts __________ in a gaseous equilibrium.
to the side with fewer moles of gas
What is the reaction quotient, Q?
Q is calculated the same way as K but for non-equilibrium concentrations.
True or false: Equilibrium can be achieved from either direction.
True, because it does not depend on the starting conditions.
What shifts equilibrium to the left?
Removing reactants or adding products shifts equilibrium to the left.
Define dynamic equilibrium.
Dynamic equilibrium is when the forward and reverse reactions occur at the same rate.
Pytania w tym zestawie(13)
1. What does an equilibrium constant K > 1 indicate?
2. Which of the following changes shifts equilibrium to the right?
3. Which is NOT a factor that affects equilibrium?
4. If Kc for a reaction is very small, what can be inferred?
5. What will happen if the volume of a container holding a gaseous equilibrium is decreased?
6. For the reaction H2(g) + I2(g) ⇌ 2HI(g), what is Kc?
7. Le Chatelier's principle implies that if the temperature is increased in an exothermic reaction, what happens?
8. What happens to the equilibrium position when a product is removed?
9. In the expression Kc = \\frac{[C]^c[D]^d}{[A]^a[B]^b}, what do [A], [B], [C], and [D] represent?
10. For a system in equilibrium, what is true about the rates of reaction?
11. What does the reaction quotient Q measure?
12. Which factor does NOT affect the equilibrium constant K?
13. If a reaction at equilibrium is disturbed, what happens?
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