Podcast
Questions and Answers
What does a negative Gibbs free energy (delta G) indicate about a reaction?
What does a negative Gibbs free energy (delta G) indicate about a reaction?
- The reaction requires energy input.
- The reaction is spontaneous. (correct)
- The reaction is at equilibrium.
- The reaction is endergonic.
A reaction with a positive delta G is described as exergonic.
A reaction with a positive delta G is described as exergonic.
False (B)
What is the Gibbs free energy when a reaction reaches equilibrium?
What is the Gibbs free energy when a reaction reaches equilibrium?
zero
A reaction that is non-spontaneous requires an input of __________.
A reaction that is non-spontaneous requires an input of __________.
Match the following terms with their definitions:
Match the following terms with their definitions:
Which term is synonymous with a spontaneous reaction?
Which term is synonymous with a spontaneous reaction?
An exergonic reaction is one that absorbs energy.
An exergonic reaction is one that absorbs energy.
What happens to the value of delta G as a reaction approaches equilibrium?
What happens to the value of delta G as a reaction approaches equilibrium?
A reaction with delta G greater than zero is considered __________.
A reaction with delta G greater than zero is considered __________.
Match the conditions with their corresponding delta G implications:
Match the conditions with their corresponding delta G implications:
What does a large equilibrium constant (K) indicate about a reaction?
What does a large equilibrium constant (K) indicate about a reaction?
Delta G can be used to indicate whether a reaction is spontaneous or non-spontaneous.
Delta G can be used to indicate whether a reaction is spontaneous or non-spontaneous.
What does the symbol 'ΔG°' represent?
What does the symbol 'ΔG°' represent?
Under standard conditions, concentrations of reactants and products are __________ molar.
Under standard conditions, concentrations of reactants and products are __________ molar.
Match the equilibrium constants with their implications:
Match the equilibrium constants with their implications:
At what temperature are standard conditions most commonly considered?
At what temperature are standard conditions most commonly considered?
A very small equilibrium constant implies many products at equilibrium.
A very small equilibrium constant implies many products at equilibrium.
What are the units for the standard Gibbs free energy change (ΔG°)?
What are the units for the standard Gibbs free energy change (ΔG°)?
Standard conditions often imply a temperature of __________ Kelvin.
Standard conditions often imply a temperature of __________ Kelvin.
If the value of K is 0.001, what does it indicate?
If the value of K is 0.001, what does it indicate?
What is the effect of a negative delta G standard on the equilibrium constant K?
What is the effect of a negative delta G standard on the equilibrium constant K?
A catalyst is consumed in the overall balanced chemical reaction.
A catalyst is consumed in the overall balanced chemical reaction.
What do we call the energy barrier that must be overcome for a reaction to proceed?
What do we call the energy barrier that must be overcome for a reaction to proceed?
At equilibrium, if delta G standard is equal to 0, the equilibrium constant K is equal to _____
At equilibrium, if delta G standard is equal to 0, the equilibrium constant K is equal to _____
Match the delta G standards with their corresponding equilibrium constants:
Match the delta G standards with their corresponding equilibrium constants:
Which statement accurately describes the function of a catalyst?
Which statement accurately describes the function of a catalyst?
A catalyst can speed up the reaction in only the forward direction.
A catalyst can speed up the reaction in only the forward direction.
What are biological catalysts in living organisms called?
What are biological catalysts in living organisms called?
A catalyst lowers the activation energy and allows a reaction to proceed _____ than it would without the catalyst.
A catalyst lowers the activation energy and allows a reaction to proceed _____ than it would without the catalyst.
Match the following terms with their definitions:
Match the following terms with their definitions:
What does a negative delta G standard indicate about a reaction?
What does a negative delta G standard indicate about a reaction?
If the equilibrium constant K is less than 1, it means the forward reaction is spontaneous.
If the equilibrium constant K is less than 1, it means the forward reaction is spontaneous.
According to the relationship between delta G standard and the equilibrium constant, what can be concluded if delta G standard is positive?
According to the relationship between delta G standard and the equilibrium constant, what can be concluded if delta G standard is positive?
In thermodynamics, under standard conditions, a delta G standard that is negative suggests that the equilibrium constant K is __________.
In thermodynamics, under standard conditions, a delta G standard that is negative suggests that the equilibrium constant K is __________.
Match the delta G standard values with their implications on reaction spontaneity:
Match the delta G standard values with their implications on reaction spontaneity:
What is the relationship between delta G standard and the natural logarithm of the equilibrium constant K?
What is the relationship between delta G standard and the natural logarithm of the equilibrium constant K?
A reaction with a delta G standard of zero is considered to be spontaneous.
A reaction with a delta G standard of zero is considered to be spontaneous.
What happens to the equilibrium constant K when delta G standard is negative?
What happens to the equilibrium constant K when delta G standard is negative?
If more reactants are present compared to products at equilibrium, then delta G standard is likely __________.
If more reactants are present compared to products at equilibrium, then delta G standard is likely __________.
Which of the following correctly describes the significance of the equilibrium constant K?
Which of the following correctly describes the significance of the equilibrium constant K?
What does a large equilibrium constant (K) indicate about a reaction?
What does a large equilibrium constant (K) indicate about a reaction?
Under standard conditions, all reactant concentrations are one molar.
Under standard conditions, all reactant concentrations are one molar.
What is the temperature commonly associated with standard conditions in Celsius?
What is the temperature commonly associated with standard conditions in Celsius?
When the equilibrium constant K is much greater than 1, the reaction favors the ______.
When the equilibrium constant K is much greater than 1, the reaction favors the ______.
Match the following equilibrium constants with their implications:
Match the following equilibrium constants with their implications:
What does a very small equilibrium constant suggest about a reaction?
What does a very small equilibrium constant suggest about a reaction?
Concentrations can be negative in equilibrium calculations.
Concentrations can be negative in equilibrium calculations.
What does the symbol 'ΔG°' represent?
What does the symbol 'ΔG°' represent?
Under standard conditions, gases are measured at a partial pressure of ______ atmosphere.
Under standard conditions, gases are measured at a partial pressure of ______ atmosphere.
Match the following delta G types with their corresponding reaction implications:
Match the following delta G types with their corresponding reaction implications:
What happens to free energy when a spontaneous reaction occurs?
What happens to free energy when a spontaneous reaction occurs?
A positive delta G indicates that a reaction is spontaneous.
A positive delta G indicates that a reaction is spontaneous.
What term is used to describe reactions that are spontaneous?
What term is used to describe reactions that are spontaneous?
When a reaction reaches equilibrium, delta G is equal to __________.
When a reaction reaches equilibrium, delta G is equal to __________.
Match the terms related to Gibbs free energy with their meanings:
Match the terms related to Gibbs free energy with their meanings:
Which of the following conditions indicates that a reaction needs energy from its surroundings?
Which of the following conditions indicates that a reaction needs energy from its surroundings?
At equilibrium, the value of delta G becomes a large negative number.
At equilibrium, the value of delta G becomes a large negative number.
What does a reaction with a negative delta G imply about its direction?
What does a reaction with a negative delta G imply about its direction?
A reaction requiring an input of energy is described as __________.
A reaction requiring an input of energy is described as __________.
Match the Gibbs free energy terms with their descriptions:
Match the Gibbs free energy terms with their descriptions:
What does a negative delta G standard indicate about the direction of a reaction?
What does a negative delta G standard indicate about the direction of a reaction?
If delta G standard is positive, then the reaction favors the products at equilibrium.
If delta G standard is positive, then the reaction favors the products at equilibrium.
What is the relationship between delta G standard and the equilibrium constant K if delta G standard is negative?
What is the relationship between delta G standard and the equilibrium constant K if delta G standard is negative?
If the natural log of K is positive, then delta G standard is __________.
If the natural log of K is positive, then delta G standard is __________.
Match the following delta G standard values with their implications:
Match the following delta G standard values with their implications:
What is the primary implication of having an equilibrium constant K less than 1?
What is the primary implication of having an equilibrium constant K less than 1?
An equilibrium constant K of 1 indicates that the reactants and products are present in equal concentrations at equilibrium.
An equilibrium constant K of 1 indicates that the reactants and products are present in equal concentrations at equilibrium.
What does a larger equilibrium constant indicate about a reaction?
What does a larger equilibrium constant indicate about a reaction?
The equation relating delta G standard to the equilibrium constant is delta G standard = __________.
The equation relating delta G standard to the equilibrium constant is delta G standard = __________.
What will happen to delta G standard if the forward reaction becomes spontaneous?
What will happen to delta G standard if the forward reaction becomes spontaneous?
What effect does a catalyst have on the activation energy of a reaction?
What effect does a catalyst have on the activation energy of a reaction?
A catalyst is consumed in the overall balanced chemical reaction.
A catalyst is consumed in the overall balanced chemical reaction.
What is the role of a catalyst in a chemical reaction?
What is the role of a catalyst in a chemical reaction?
Enzymes are biological __________ that speed up reactions in living organisms.
Enzymes are biological __________ that speed up reactions in living organisms.
Match the following terms with their correct definitions:
Match the following terms with their correct definitions:
When delta G standard is 0, what is the value of the equilibrium constant (K)?
When delta G standard is 0, what is the value of the equilibrium constant (K)?
A catalyst speeds up the reaction only in the forward direction.
A catalyst speeds up the reaction only in the forward direction.
What condition is generally required for delta G standard to indicate a spontaneous reaction?
What condition is generally required for delta G standard to indicate a spontaneous reaction?
The energy barrier that must be overcome for a reaction to proceed is called the __________.
The energy barrier that must be overcome for a reaction to proceed is called the __________.
What is a common characteristic of a reaction with a positive delta G standard?
What is a common characteristic of a reaction with a positive delta G standard?
Study Notes
Thermodynamics and Kinetics Overview
- Gibbs free energy (ΔG) determines spontaneity of reactions; negative ΔG indicates spontaneous reactions, known as exergonic.
- Exergonic reactions proceed downhill in free energy; they release energy to do work.
- Non-spontaneous reactions (positive ΔG) are referred to as endergonic, requiring energy input from surroundings to proceed.
- Reactions proceed spontaneously until equilibrium is reached, indicated by ΔG equaling zero.
Gibbs Free Energy and Equilibrium
- Standard conditions for ΔG: all reactant concentrations at 1 M, gases at 1 atm, and typically 25°C (298 K).
- The equilibrium constant (K) represents the concentration ratio of products to reactants at equilibrium.
- A large K (greater than 1, especially above 1000) indicates a reaction that favors products.
- A small K (less than 1) shows a reaction that favors reactants; K cannot be negative as concentrations are non-negative.
- K around 1 suggests a balanced reaction with significant amounts of both products and reactants.
Relationship Between ΔG and K
- The equation ΔG° = -RT ln K relates standard Gibbs free energy to the equilibrium constant.
- Negative ΔG° indicates a spontaneous reaction under standard conditions, resulting in K > 1 (favoring products).
- Positive ΔG° signifies a non-spontaneous reaction, leading to K < 1 (favoring reactants).
- When ΔG° = 0, the equilibrium constant K equals 1, which is a rare occurrence.
Catalysts and Enzymes
- Catalysts speed up reactions by providing an alternative pathway with lower activation energy.
- Lower activation energy allows reactions to proceed more quickly, affecting both forward and reverse directions.
- Catalysts are not consumed in the overall reaction and can facilitate multiple reactions without being depleted.
- Enzymes function as biological catalysts, repeating the process for successive reactions in living organisms.
Thermodynamics and Kinetics Overview
- Gibbs free energy (ΔG) determines spontaneity of reactions; negative ΔG indicates spontaneous reactions, known as exergonic.
- Exergonic reactions proceed downhill in free energy; they release energy to do work.
- Non-spontaneous reactions (positive ΔG) are referred to as endergonic, requiring energy input from surroundings to proceed.
- Reactions proceed spontaneously until equilibrium is reached, indicated by ΔG equaling zero.
Gibbs Free Energy and Equilibrium
- Standard conditions for ΔG: all reactant concentrations at 1 M, gases at 1 atm, and typically 25°C (298 K).
- The equilibrium constant (K) represents the concentration ratio of products to reactants at equilibrium.
- A large K (greater than 1, especially above 1000) indicates a reaction that favors products.
- A small K (less than 1) shows a reaction that favors reactants; K cannot be negative as concentrations are non-negative.
- K around 1 suggests a balanced reaction with significant amounts of both products and reactants.
Relationship Between ΔG and K
- The equation ΔG° = -RT ln K relates standard Gibbs free energy to the equilibrium constant.
- Negative ΔG° indicates a spontaneous reaction under standard conditions, resulting in K > 1 (favoring products).
- Positive ΔG° signifies a non-spontaneous reaction, leading to K < 1 (favoring reactants).
- When ΔG° = 0, the equilibrium constant K equals 1, which is a rare occurrence.
Catalysts and Enzymes
- Catalysts speed up reactions by providing an alternative pathway with lower activation energy.
- Lower activation energy allows reactions to proceed more quickly, affecting both forward and reverse directions.
- Catalysts are not consumed in the overall reaction and can facilitate multiple reactions without being depleted.
- Enzymes function as biological catalysts, repeating the process for successive reactions in living organisms.
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Description
Explore the principles of thermodynamics and kinetics, focusing on Gibbs free energy and its implications for reaction spontaneity. Understand the concepts of exergonic and endergonic reactions, equilibrium, and the significance of the equilibrium constant. This quiz is perfect for students looking to solidify their grasp of these fundamental concepts in chemistry.
