Podcast
Questions and Answers
The half-life of a first order reaction is _____ of the concentration of reactants.
The half-life of a first order reaction is _____ of the concentration of reactants.
independent
An increase in the number of molecular collisions generally _____ the rate of reaction.
An increase in the number of molecular collisions generally _____ the rate of reaction.
increases
The _____ state is a high-energy state that occurs during the transition from reactants to products.
The _____ state is a high-energy state that occurs during the transition from reactants to products.
transition
Catalysts work by lowering the _____ energy required for a reaction, thus increasing the rate constant.
Catalysts work by lowering the _____ energy required for a reaction, thus increasing the rate constant.
At equilibrium, the forward rate of a reaction is _____ to the reverse rate.
At equilibrium, the forward rate of a reaction is _____ to the reverse rate.
The equilibrium constant, K, is influenced by the _____ of reactants and products.
The equilibrium constant, K, is influenced by the _____ of reactants and products.
Buffers can resist changes in _____ when acids or bases are added.
Buffers can resist changes in _____ when acids or bases are added.
In an ICE table, the letters I, C, and E stand for Initial, Change, and _____ respectively.
In an ICE table, the letters I, C, and E stand for Initial, Change, and _____ respectively.
The addition of a catalyst affects the _____ of a reaction but does not change the equilibrium position.
The addition of a catalyst affects the _____ of a reaction but does not change the equilibrium position.
When a salt dissolves in water, the _____ of the resulting solution can change due to the dissociation of ions.
When a salt dissolves in water, the _____ of the resulting solution can change due to the dissociation of ions.
A chemical reaction that absorbs heat is classified as ______.
A chemical reaction that absorbs heat is classified as ______.
The heat capacity of a substance indicates how much heat is needed to raise its temperature by one degree, known as ______.
The heat capacity of a substance indicates how much heat is needed to raise its temperature by one degree, known as ______.
In a calorimeter, the relationship ______ represents the conservation of energy principle.
In a calorimeter, the relationship ______ represents the conservation of energy principle.
The change in enthalpy is represented by the symbol ______.
The change in enthalpy is represented by the symbol ______.
The entropy change of a reaction is represented by ______.
The entropy change of a reaction is represented by ______.
At equilibrium, the entropy change of the reaction (Sºrxn) is ______.
At equilibrium, the entropy change of the reaction (Sºrxn) is ______.
The law that states energy cannot be created or destroyed is known as the ______ law of thermodynamics.
The law that states energy cannot be created or destroyed is known as the ______ law of thermodynamics.
The process by which substances dissolve involves changes in enthalpy (ΔH) and ______.
The process by which substances dissolve involves changes in enthalpy (ΔH) and ______.
Energy changes in reactions arise from changes in ______ energies.
Energy changes in reactions arise from changes in ______ energies.
Chemical reactions involve rearrangements of ______ to produce new chemical species.
Chemical reactions involve rearrangements of ______ to produce new chemical species.
The relationship between [–OH] and [H3O+] in aqueous solution is critical for understanding acid-base chemistry, especially in determining the pH.
The relationship between [–OH] and [H3O+] in aqueous solution is critical for understanding acid-base chemistry, especially in determining the pH.
A solution is defined as acidic, basic, or neutral using the ______ scale.
A solution is defined as acidic, basic, or neutral using the ______ scale.
The extent of a reaction is related to the ______ energy change from reactants to products.
The extent of a reaction is related to the ______ energy change from reactants to products.
Acid-base reactions can be classified based on the behavior of ______ electrons.
Acid-base reactions can be classified based on the behavior of ______ electrons.
The position of equilibrium can be changed by altering the ______ of reactants or products.
The position of equilibrium can be changed by altering the ______ of reactants or products.
Bronsted-Lowry acids and bases are defined by their ability to donate or accept ______.
Bronsted-Lowry acids and bases are defined by their ability to donate or accept ______.
A solution that can resist changes in pH when small amounts of acid or base are added is known as a ______.
A solution that can resist changes in pH when small amounts of acid or base are added is known as a ______.
The phenomenon where a salt dissociates in water and causes a change in pH is related to its ______.
The phenomenon where a salt dissociates in water and causes a change in pH is related to its ______.
In an acid-base titration, the point at which the amount of acid equals the amount of base is called the ______.
In an acid-base titration, the point at which the amount of acid equals the amount of base is called the ______.
When weak acids react with strong bases, they form ______ in a titration curve.
When weak acids react with strong bases, they form ______ in a titration curve.
Buffer capacity is defined as the ability of a buffer to ______ changes in pH upon the addition of an acid or a base.
Buffer capacity is defined as the ability of a buffer to ______ changes in pH upon the addition of an acid or a base.
The ______ of a chemical reaction describes how quickly reactants are converted into products.
The ______ of a chemical reaction describes how quickly reactants are converted into products.
Increased ______ typically leads to an increase in the rate of reaction by providing more reactant molecules to collide.
Increased ______ typically leads to an increase in the rate of reaction by providing more reactant molecules to collide.
The ______ constant (K) can be calculated using the concentrations of reactants and products at equilibrium.
The ______ constant (K) can be calculated using the concentrations of reactants and products at equilibrium.
In first order reactions, the ______ can be defined as the time it takes for the concentration of a reactant to reduce to half its initial value.
In first order reactions, the ______ can be defined as the time it takes for the concentration of a reactant to reduce to half its initial value.
A catalyst works by lowering the ______ of a reaction, making it easier for reactants to convert into products.
A catalyst works by lowering the ______ of a reaction, making it easier for reactants to convert into products.
The ______ law provides a mathematical expression that relates the rate of a reaction to the concentration of its reactants.
The ______ law provides a mathematical expression that relates the rate of a reaction to the concentration of its reactants.
The state of ______ equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
The state of ______ equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction.
The ______ of a reaction can be determined by analyzing the concentration versus time data through graphing.
The ______ of a reaction can be determined by analyzing the concentration versus time data through graphing.
Flashcards
Specific Heat Capacity
Specific Heat Capacity
The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius.
Exothermic Reaction
Exothermic Reaction
A reaction that releases heat into the surroundings. The enthalpy change, ΔH, is negative.
Endothermic Reaction
Endothermic Reaction
A reaction that absorbs heat from the surroundings. The enthalpy change, ΔH, is positive.
Enthalpy Change (ΔH)
Enthalpy Change (ΔH)
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Enthalpy Diagram
Enthalpy Diagram
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Heat of Reaction (ΔHrxn)
Heat of Reaction (ΔHrxn)
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Heat of Formation (ΔHf)
Heat of Formation (ΔHf)
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Standard Heat of Formation Reaction
Standard Heat of Formation Reaction
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Half-life (t1/2)
Half-life (t1/2)
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Activation Energy (Ea)
Activation Energy (Ea)
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Transition State
Transition State
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Catalyst
Catalyst
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Equilibrium Constant (K)
Equilibrium Constant (K)
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What is a neutralization reaction?
What is a neutralization reaction?
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What is a redox reaction?
What is a redox reaction?
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What is a Brønsted-Lowry acid?
What is a Brønsted-Lowry acid?
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What is a Brønsted-Lowry base?
What is a Brønsted-Lowry base?
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What are amphoteric substances?
What are amphoteric substances?
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What is the activation energy?
What is the activation energy?
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How do changes in reactant and product concentrations affect the position of equilibrium?
How do changes in reactant and product concentrations affect the position of equilibrium?
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What is the equilibrium constant (K)?
What is the equilibrium constant (K)?
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Buffer
Buffer
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Coupled Reactions
Coupled Reactions
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Buffer Capacity
Buffer Capacity
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pH of Salt Solutions
pH of Salt Solutions
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Acid-Base Buffer
Acid-Base Buffer
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Common-Ion Effect
Common-Ion Effect
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Buffer Range
Buffer Range
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Reaction Rate
Reaction Rate
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Factors Affecting Reaction Rate
Factors Affecting Reaction Rate
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Rate Law
Rate Law
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Reaction Order
Reaction Order
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Rate Constant (k)
Rate Constant (k)
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Half-Life
Half-Life
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Dynamic Equilibrium
Dynamic Equilibrium
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Study Notes
General Chemistry Concepts
- Chemical reactions involve rearrangements of atoms to create new chemical species with different properties.
- Chemical reactions involve changes in the arrangement of atomic cores and valence electrons.
- Reactions can be classified based on how valence electrons behave (e.g., acid-base, redox).
- Energy changes in reactions result from breaking and forming bonds.
Thermochemistry
- The temperature at which a phase change occurs depends on molecular structure.
- For molecular substances, intermolecular forces are overcome during phase changes, not chemical bonds.
- Phase changes' direction depends on an increase in total entropy or Gibbs free energy (ΔG).
- Temperature, thermal energy, and kinetic energy are related.
- Kinetic energy varies among particles at the same temperature, based on factors like molecular weight.
- Heating/cooling curves show temperature changes when thermal energy is added (or removed), including phase changes.
- Temperature remains constant during phase changes.
- Open, closed, and isolated systems differ in matter exchange with the surroundings.
- State functions (like enthalpy) are independent of path.
Thermodynamics
- Entropy (S) and free energy (G) are thermodynamic properties.
- The sign of ΔG predicts whether a process is thermodynamically favorable.
- The second law of thermodynamics relates to entropy increases in the universe.
- Understanding ΔH and ΔS is key to determining favorability.
- Spontaneity is not always related to speed.
- Equilibrium is a balance between forward and reverse reaction rates.
Solutions
- Solutions are stable mixtures at the molecular level.
- Solubility is affected by enthalpy and entropy changes. "Like dissolves like" is a general guideline.
- Solute, solvent, and solution terms should be understood.
- Concentrations are measured using different units (e.g., molarity, molality, percent by mass).
- Temperature affects solubility.
- Interactions between solute and solvent particles are central to solution formation.
Reaction Rates and Equilibrium
- Reaction rates depend on activation energy and the probability of molecules colliding with sufficient energy.
- Reaction rates are influenced by temperature, concentration, catalysts, and other factors.
- Equilibrium is a balance between forward and reverse reactions and can be influenced by external factors.
- Reaction rate, equilibrium constant, and rate laws should be understood in relation to each other.
- Equilibrium shifts in response to stress (Le Chatelier's principle). Activation energy and transition states determine reaction rates.
Acids and Bases
- Arrhenius, Brønsted-Lowry, and Lewis acid-base definitions exist.
- Acid-base reactions involve proton transfer (or electron pair acceptance).
- Equilibrium considerations are key when acids and bases react .
- The strength of an acid or base affects the extent and nature of reactions.
- pH and pOH are measures of acidity and basicity.
- Buffers resist pH changes.
Additional Concepts
- Calorimetry is used to measure heat changes.
- Spectroscopic measurements are used to study molecules.
- Stoichiometry is applied to balance and predict reactions.
- Calculations are essential in solving chemistry problems.
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Description
Test your understanding of key concepts in chemistry, including reaction rates, equilibrium, and thermodynamics, through this quiz. Explore the fundamental principles that govern chemical reactions and the role of catalysts and buffers. Perfect for students studying chemistry at an advanced level.
