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Questions and Answers
What is the correct term for a reaction that involves an exchange of cations between two compounds in solution?
What is the correct term for a reaction that involves an exchange of cations between two compounds in solution?
Which direction represents the formation in the equilibrium reaction A + B ↔ C + D?
Which direction represents the formation in the equilibrium reaction A + B ↔ C + D?
What occurs to the concentration of reactants as a reaction approaches equilibrium?
What occurs to the concentration of reactants as a reaction approaches equilibrium?
At equilibrium, the rates of which of the following are equal?
At equilibrium, the rates of which of the following are equal?
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Which statement about the amount of reactants and products at equilibrium is true?
Which statement about the amount of reactants and products at equilibrium is true?
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What is defined as the change in concentration of a reactant or product per unit time?
What is defined as the change in concentration of a reactant or product per unit time?
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When a system at equilibrium is disturbed, what is expected to happen?
When a system at equilibrium is disturbed, what is expected to happen?
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What term describes a state where concentrations of reactants and products remain constant?
What term describes a state where concentrations of reactants and products remain constant?
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What factor does NOT affect the rate of a chemical reaction?
What factor does NOT affect the rate of a chemical reaction?
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Which statement accurately describes the Law of Mass Action?
Which statement accurately describes the Law of Mass Action?
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If the molar concentrations of reactants A and B are both 2 M, what can be inferred about the reaction rate?
If the molar concentrations of reactants A and B are both 2 M, what can be inferred about the reaction rate?
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What is the equilibrium constant represented in the equation?
What is the equilibrium constant represented in the equation?
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What happens to the reaction rate when the concentration of reactants increases?
What happens to the reaction rate when the concentration of reactants increases?
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Which of the following statements is true regarding covalently bonded molecules in reactions?
Which of the following statements is true regarding covalently bonded molecules in reactions?
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Which term defines the rate of a reaction in which the concentration of reactants is at 1 M?
Which term defines the rate of a reaction in which the concentration of reactants is at 1 M?
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What is the likely outcome when physical nature of the medium of reaction changes?
What is the likely outcome when physical nature of the medium of reaction changes?
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What is the relationship between the equilibrium constant Keq and the concentrations of reactants and products at equilibrium?
What is the relationship between the equilibrium constant Keq and the concentrations of reactants and products at equilibrium?
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What happens to the equilibrium when the pressure is increased in a reaction where 4 moles of gas convert to 2 moles of gas?
What happens to the equilibrium when the pressure is increased in a reaction where 4 moles of gas convert to 2 moles of gas?
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According to Le Chatelier’s principle, what is expected when the concentration of reactant A is increased?
According to Le Chatelier’s principle, what is expected when the concentration of reactant A is increased?
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If Keq is greater than 1, what can be inferred about the reaction?
If Keq is greater than 1, what can be inferred about the reaction?
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How does the addition of HCl affect the ionization of acetic acid?
How does the addition of HCl affect the ionization of acetic acid?
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Which statement about the effect of catalysts on Keq is true?
Which statement about the effect of catalysts on Keq is true?
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What is the effect of adding AgNO3 to a saturated solution of AgCl?
What is the effect of adding AgNO3 to a saturated solution of AgCl?
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How does Le Chatelier's Principle describe the response of a system at equilibrium when a stress is applied?
How does Le Chatelier's Principle describe the response of a system at equilibrium when a stress is applied?
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In an exothermic reaction, what happens when energy is added?
In an exothermic reaction, what happens when energy is added?
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Which of the following scenarios would not result in a shift of equilibrium?
Which of the following scenarios would not result in a shift of equilibrium?
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What effect does the common ion effect have on weak acids or bases?
What effect does the common ion effect have on weak acids or bases?
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Which factor does not influence the equilibrium position of a reaction?
Which factor does not influence the equilibrium position of a reaction?
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If the concentration of a product is increased, what is the expected effect on the equilibrium position?
If the concentration of a product is increased, what is the expected effect on the equilibrium position?
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For a reaction involving gases, how does an increase in pressure affect the equilibrium position?
For a reaction involving gases, how does an increase in pressure affect the equilibrium position?
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Which reaction demonstrates no change in total moles of gas during pressure alteration?
Which reaction demonstrates no change in total moles of gas during pressure alteration?
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What is true about the equilibrium constant's dependence on temperature?
What is true about the equilibrium constant's dependence on temperature?
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Study Notes
Introduction to General Inorganic Chemistry
- Pharmaceutical Analytical Chemistry I (PC 111), Level I, Pharm D Clinical
- Lecture 6
- Presented by Dr. Galal Magdy, PhD
Metathesis Reactions
- Metathesis (double replacement) reactions involve two compounds in solution, exchanging cations with anions
- Example: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
Chemical Equilibrium
- A chemical reaction has a forward and a backward reaction
- Products of a reaction interact to form reactants
- This occurs simultaneously in both directions
- Reaction rates change as the reaction progresses
- Equilibrium occurs when forward reaction rate equals reverse reaction rate
- At equilibrium, concentrations of reactants and products remain constant
Dynamic Equilibrium
- A state of equilibrium where the forward and backward reaction rates are equal, yet there is continuous exchange of products and reactants
- Concentrations of reactants and products are constant
Reaction Rate
- Reaction rate = change in reactant/product concentration per unit time
- Some reactions are fast, others are slow
- Generally, ion-based reactions are rapid
- Covalent reactions are often slower
- Examples:
- Rapid: Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
- Slow: Iron to iron oxide (rust)
Factors Affecting Reaction Rate
- Nature of reactants
- Reactant concentration
- Pressure (gaseous systems)
- Temperature
- Catalysts
- Physical nature of reaction medium
Effect of Concentration on Reaction Rate
- Collisions between ions or molecules lead to product formation
- Increasing the number of reactant moles increases collision chances, thus increasing reaction rate
- The law describing concentration's effect on reaction rate is the Law of Mass Action (Law of Chemical Equilibrium)
- Reaction rate is directly proportional to the active masses (molar concentrations) of reacting substances
Rate Constant
- The rate constant (k) is the proportionality constant relating the rate of a reaction to the concentrations of reactants
- If reactant concentrations are 1 M, the rate equals the rate constant
- Rate = k[A]m[B]n
Equilibrium Constant (Keq)
- The equilibrium constant (Keq) is the ratio of the rate constant for the forward reaction (k₁) to the rate constant for the reverse reaction (k₂) at equilibrium
- The ratio is equal to the molar concentration of products raised to their respective stoichiometric coefficients divided by a similar term for reactants Keq = ([C]c[D]d)/([A]a[B]b)
Factors Affecting Keq
- Keq is not affected by catalysts, concentration changes, or equilibrium position changes
- Keq is affected only by temperature and pressure and depends on reactant nature
Le Chatelier's Principle
- When a stress is applied to a system in equilibrium, the equilibrium shifts in a direction that neutralizes the stress
- Factors affecting the reaction equilibrium: temperature, pressure, and concentration
Temperature
- Exothermic reaction: Adding energy shifts equilibrium to the left
- Endothermic reaction: Adding energy shifts equilibrium to the right
Pressure
- Pressure affects equilibrium only if one or more reactants or products are gases
- Increasing pressure shifts equilibrium towards the side with fewer moles of gas
Concentration
- Increasing reactant concentration shifts equilibrium to the right
- Increasing product concentration shifts equilibrium to the left
Common Ion Effect
- Adding a strong electrolyte with a common ion to a solution of a weak electrolyte decreases the concentration of the common ion
- It suppresses the ionization of weak acids or bases
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Description
This quiz covers key concepts from Lecture 6 of Pharmaceutical Analytical Chemistry I. It focuses on metathesis reactions, chemical equilibrium, and dynamic equilibrium, providing examples and explanations to enhance your understanding. Test your knowledge on these fundamental topics essential for a Clinical Pharm D program.
