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Questions and Answers
What is a key characteristic of dynamic equilibrium?
What is a key characteristic of dynamic equilibrium?
- There are no particles in motion.
- The system is closed, and reactions occur at the same rate. (correct)
- The system is open to matter exchange.
- Only forward reactions occur.
Static equilibrium is characterized by constant motion of particles.
Static equilibrium is characterized by constant motion of particles.
False (B)
What principle states that a system will counteract changes made to it in order to restore equilibrium?
What principle states that a system will counteract changes made to it in order to restore equilibrium?
Le Chatelier's Principle
In the equation for chemical equilibrium, Kc represents the __________ of reactants to products.
In the equation for chemical equilibrium, Kc represents the __________ of reactants to products.
Match the type of equilibrium with its example:
Match the type of equilibrium with its example:
Which of the following statements is true regarding Kp and Kc?
Which of the following statements is true regarding Kp and Kc?
Increasing pressure in a reaction favors the side with higher moles of gas.
Increasing pressure in a reaction favors the side with higher moles of gas.
What happens to the equilibrium position of the Haber Process if the temperature is lowered?
What happens to the equilibrium position of the Haber Process if the temperature is lowered?
What does a catalyst do in a chemical reaction?
What does a catalyst do in a chemical reaction?
Temperature can influence the equilibrium constant.
Temperature can influence the equilibrium constant.
What is the equilibrium constant (Keq) for the reaction CO(g) + H2O(g) ↔ CO2(g) + H2(g) at 600 K?
What is the equilibrium constant (Keq) for the reaction CO(g) + H2O(g) ↔ CO2(g) + H2(g) at 600 K?
At equilibrium, the concentration of CO and H2O will be ______ M.
At equilibrium, the concentration of CO and H2O will be ______ M.
Match the following reactions with their characteristics:
Match the following reactions with their characteristics:
What is represented by the variable x in the calculations for equilibrium?
What is represented by the variable x in the calculations for equilibrium?
A catalyst alters the equilibrium constant of a reaction.
A catalyst alters the equilibrium constant of a reaction.
To find the molar concentration, one must divide the number of moles by the ________.
To find the molar concentration, one must divide the number of moles by the ________.
What is the equilibrium constant (K) expression for the reaction H2(g) + I2(g) ⇌ 2 HI(g)?
What is the equilibrium constant (K) expression for the reaction H2(g) + I2(g) ⇌ 2 HI(g)?
The equilibrium constant (K) can change if the temperature of the system is altered.
The equilibrium constant (K) can change if the temperature of the system is altered.
Calculate the equilibrium constant (K) if the equilibrium concentrations of NO2 and N2O4 are 0.4 and 0.2 mol dm-3 respectively.
Calculate the equilibrium constant (K) if the equilibrium concentrations of NO2 and N2O4 are 0.4 and 0.2 mol dm-3 respectively.
In a 1.00-L container of phosgene, if the concentration of Cl2 is 0.028 M, the concentration of CO will be _____ M.
In a 1.00-L container of phosgene, if the concentration of Cl2 is 0.028 M, the concentration of CO will be _____ M.
If the equilibrium constant (Kc) for H2(g) + I2(g) ⇌ 2 HI(g) is given as 50.3 at 731 K, what will happen if the concentrations of H2 and I2 are both introduced at 0.100 M?
If the equilibrium constant (Kc) for H2(g) + I2(g) ⇌ 2 HI(g) is given as 50.3 at 731 K, what will happen if the concentrations of H2 and I2 are both introduced at 0.100 M?
The equilibrium constant (Kp) has a different expression from Kc for the same reaction.
The equilibrium constant (Kp) has a different expression from Kc for the same reaction.
What is the value of K if the equilibrium concentrations of the reactants and products lead to a K value greater than 1?
What is the value of K if the equilibrium concentrations of the reactants and products lead to a K value greater than 1?
During the decomposition of COCl2(g) to CO(g) and Cl2(g), the initial concentration of COCl2 was _____ M.
During the decomposition of COCl2(g) to CO(g) and Cl2(g), the initial concentration of COCl2 was _____ M.
Match the following equilibrium constants with their types:
Match the following equilibrium constants with their types:
What is the equilibrium expression $K_c$ for the reaction $4NH_3 + 5O_2 ↔ 4NO + 6H_2O$?
What is the equilibrium expression $K_c$ for the reaction $4NH_3 + 5O_2 ↔ 4NO + 6H_2O$?
The addition of more iodine will shift the equilibrium reaction to the right.
The addition of more iodine will shift the equilibrium reaction to the right.
What colour would be observed if the equilibrium position is on the right?
What colour would be observed if the equilibrium position is on the right?
If the temperature of the system is increased and the forward reaction is exothermic, the system will try to ________.
If the temperature of the system is increased and the forward reaction is exothermic, the system will try to ________.
What will happen if the pressure of the system with 2NO2 (brown gas) and N2O4 (colourless gas) is increased?
What will happen if the pressure of the system with 2NO2 (brown gas) and N2O4 (colourless gas) is increased?
Decreasing the temperature favors the forward reaction in an exothermic equilibrium.
Decreasing the temperature favors the forward reaction in an exothermic equilibrium.
What colour would likely be observed if the pressure is increased in the reaction between NO2 and N2O4?
What colour would likely be observed if the pressure is increased in the reaction between NO2 and N2O4?
A catalyst affects the rate of the forward reaction only, True or ________.
A catalyst affects the rate of the forward reaction only, True or ________.
In the event of adding more reactants to a system at equilibrium, what generally occurs?
In the event of adding more reactants to a system at equilibrium, what generally occurs?
The reaction $2NO_2 ↔ N_2O_4$ has a negative $ riangle H$, indicating it is endothermic.
The reaction $2NO_2 ↔ N_2O_4$ has a negative $ riangle H$, indicating it is endothermic.
What would be the effect on the equilibrium when a catalyst is added?
What would be the effect on the equilibrium when a catalyst is added?
In an exothermic reaction, increasing the temperature shifts the equilibrium to the ________.
In an exothermic reaction, increasing the temperature shifts the equilibrium to the ________.
What would be the expected observation if the equilibrium position is on the left for a given reaction?
What would be the expected observation if the equilibrium position is on the left for a given reaction?
Match the reaction conditions to the expected outcomes:
Match the reaction conditions to the expected outcomes:
Flashcards
Chemical Equilibrium
Chemical Equilibrium
A state where the rate of the forward reaction equals the rate of the reverse reaction, leading to no net change in the concentrations of reactants and products.
Static Equilibrium
Static Equilibrium
A type of equilibrium where there is no movement or change in the system. It is a static and unchanging condition.
Dynamic Equilibrium
Dynamic Equilibrium
A type of equilibrium where there is continuous movement and change, but the overall system remains balanced. The rates of the forward and reverse reactions are equal.
Equilibrium Constant (Kc)
Equilibrium Constant (Kc)
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Le Chatelier's Principle
Le Chatelier's Principle
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Temperature Effect on Equilibrium
Temperature Effect on Equilibrium
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Pressure Effect on Equilibrium
Pressure Effect on Equilibrium
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Concentration Effect on Equilibrium
Concentration Effect on Equilibrium
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Change (x)
Change (x)
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ICE Table
ICE Table
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Initial Conditions
Initial Conditions
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Equilibrium Conditions
Equilibrium Conditions
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Catalyst
Catalyst
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Equilibrium
Equilibrium
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Equilibrium Constant (Keq) at a specific temperature
Equilibrium Constant (Keq) at a specific temperature
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What is the Equilibrium Constant (Kc)?
What is the Equilibrium Constant (Kc)?
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What's the Kc expression for 4NH3 + 5O2 ↔ 4NO + 6H2O?
What's the Kc expression for 4NH3 + 5O2 ↔ 4NO + 6H2O?
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Will the equilibrium shift left or right if more iodine is added?
Will the equilibrium shift left or right if more iodine is added?
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What color will the solution be when more iodine is added?
What color will the solution be when more iodine is added?
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How will the equilibrium shift if the temperature is increased?
How will the equilibrium shift if the temperature is increased?
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What does a catalyst do to the equilibrium position?
What does a catalyst do to the equilibrium position?
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If the pressure is increased for 2NO2 (brown gas) ↔ N2O4 (colorless gas), what color would be seen?
If the pressure is increased for 2NO2 (brown gas) ↔ N2O4 (colorless gas), what color would be seen?
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If the temperature is decreased for 2NO2 (brown gas) ↔ N2O4 (colorless gas), which reaction will be favored?
If the temperature is decreased for 2NO2 (brown gas) ↔ N2O4 (colorless gas), which reaction will be favored?
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Equilibrium Constant (K) and Free Energy (ΔG)
Equilibrium Constant (K) and Free Energy (ΔG)
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Equilibrium constant
Equilibrium constant
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Kp
Kp
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Study Notes
Equilibrium
- Equilibrium is a state where the forward and reverse reactions occur at the same rate.
- Two types of equilibrium: static and dynamic.
- Static equilibrium: Two equal weights on a seesaw.
- Dynamic equilibrium: A restaurant with constant occupancy despite people entering and leaving.
Characteristics of Dynamic Equilibrium
- Closed system: No matter enters or exits.
- Constant rate: The forward and reverse reactions occur at the same rate.
- Macroscopic scale: No noticeable change.
- Microscopic scale: Constant motion of particles.
Principles of Chemical Equilibrium
- Equilibrium constant (K): The ratio of product concentrations to reactant concentrations at a given temperature.
- General reaction: aA + bB ⇌ cC + dD
- Equilibrium constant expression: K = [C]c[D]d / [A]a[B]b
- represents concentration.
- Kp: Equilibrium constant in terms of partial pressures (for gases only). Solids are excluded.
- Example: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
Le Chatelier's Principle
- If a change (stressor) is applied to a system in equilibrium, the system will shift to counteract the change and re-establish equilibrium.
- Examples: Change in temperature, pressure, or concentration.
Catalyst
- Catalysts speed up the rate of both forward and reverse reactions.
- They do not shift the equilibrium position or the equilibrium constant.
- They only affect the rate at which equilibrium is reached.
Temperature Changes
- Temperature affects the equilibrium constant.
Pressure Changes
- If pressure increases, the equilibrium shifts towards the side with fewer moles of gas to reduce pressure.
- If pressure decreases, the equilibrium shifts towards the side with more moles of gas to increase pressure.
Haber Process
- N₂ + 3H₂ ⇌ 2NH₃ ΔH is -ve, meaning the forward reaction is exothermic.
- Lowering the temperature favors the exothermic forward reaction thus increasing the yield of ammonia.
- Increasing pressure favors the side with fewer moles of gas (the right side), also increases the ammonia yield.
Contact Process
- Similar to Haber process, system shifts to counteract applied pressure change.
Equilibrium Calculations
- ICE tables (Initial, Change, Equilibrium) are useful tools for calculating equilibrium concentrations.
- Used to solve for unknown quantities upon adding reactants or products to existing equilibrium conditions.
Equilibrium Constant, Kc
- Equilibrium constant for a given reaction at a defined temperature.
- Used to determine how much reactants/products are at equilibrium.
- Value determined based on amounts of products/reactants.
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