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Questions and Answers
What is the molecularity of the reaction represented by PCL₃ + CL₂ -> PCL₅?
What is the molecularity of the reaction represented by PCL₃ + CL₂ -> PCL₅?
If the rate law for a reaction is given by ROR = K[A]²[B], what is the order of the reaction?
If the rate law for a reaction is given by ROR = K[A]²[B], what is the order of the reaction?
Which of the following statements about order of reaction is true?
Which of the following statements about order of reaction is true?
What happens to the rate of reaction (ROR) if the concentration of A is halved while keeping B constant, given that the order with respect to A is 2?
What happens to the rate of reaction (ROR) if the concentration of A is halved while keeping B constant, given that the order with respect to A is 2?
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Which of the following is a correct statement regarding the relationship between concentration and order of reaction?
Which of the following is a correct statement regarding the relationship between concentration and order of reaction?
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What is the relationship described by the Rate law?
What is the relationship described by the Rate law?
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Which condition is NOT required for an effective collision to occur?
Which condition is NOT required for an effective collision to occur?
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Increasing temperature affects the rate of reaction by...
Increasing temperature affects the rate of reaction by...
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Which of the following describes the Arrhenius equation in terms of temperature?
Which of the following describes the Arrhenius equation in terms of temperature?
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Which factor does NOT directly affect the rate of reaction according to collision theory?
Which factor does NOT directly affect the rate of reaction according to collision theory?
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In the context of the Arrhenius equation, what does 'A' represent?
In the context of the Arrhenius equation, what does 'A' represent?
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How is molecularity defined in the context of a chemical reaction?
How is molecularity defined in the context of a chemical reaction?
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What effect does a positive catalyst have on the rate of reaction?
What effect does a positive catalyst have on the rate of reaction?
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What is the definition of the rate of reaction?
What is the definition of the rate of reaction?
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How is the instantaneous rate of reaction denoted in mathematical terms?
How is the instantaneous rate of reaction denoted in mathematical terms?
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What does the law of mass action state about the rate of reaction?
What does the law of mass action state about the rate of reaction?
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Which of the following is true about the rate constant (K)?
Which of the following is true about the rate constant (K)?
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In the reaction A + 2B -> 3C, how would you express the rate of reaction with respect to d[C]/dt?
In the reaction A + 2B -> 3C, how would you express the rate of reaction with respect to d[C]/dt?
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What is the characteristic of an elementary reaction compared to a complex reaction?
What is the characteristic of an elementary reaction compared to a complex reaction?
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What role does concentration play in the rate of reaction?
What role does concentration play in the rate of reaction?
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In the expression R.O.R = K[A][B], what do A and B represent?
In the expression R.O.R = K[A][B], what do A and B represent?
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Which of the following statements correctly describes a first-order reaction?
Which of the following statements correctly describes a first-order reaction?
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How is pseudo first-order reaction defined?
How is pseudo first-order reaction defined?
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What is the relationship of the half-life of a first-order reaction to the rate constant?
What is the relationship of the half-life of a first-order reaction to the rate constant?
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In the context of a pseudo first-order reaction, what is the role of the excess reactant?
In the context of a pseudo first-order reaction, what is the role of the excess reactant?
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What is indicated by the equation Kt = 2.303 log₁₀ (a₀/x) for a first-order reaction?
What is indicated by the equation Kt = 2.303 log₁₀ (a₀/x) for a first-order reaction?
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Which graph accurately represents a first-order reaction?
Which graph accurately represents a first-order reaction?
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What does τ = ∞ imply for a first-order reaction?
What does τ = ∞ imply for a first-order reaction?
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Which of the following is NOT a characteristic of a solution?
Which of the following is NOT a characteristic of a solution?
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What is the unit of molality in a solution?
What is the unit of molality in a solution?
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Which of the following statements is true regarding molarity and molality?
Which of the following statements is true regarding molarity and molality?
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If 5 moles of NaCl are dissolved in 2 kg of water, what is the molality of the solution?
If 5 moles of NaCl are dissolved in 2 kg of water, what is the molality of the solution?
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What does mole fraction represent in a solution?
What does mole fraction represent in a solution?
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Which of the following is not a method to express concentration of solutions?
Which of the following is not a method to express concentration of solutions?
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What is the molarity of a solution if 0.3 moles of solute are present in 0.5 liters?
What is the molarity of a solution if 0.3 moles of solute are present in 0.5 liters?
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According to Henry's law, what happens to the solubility of gas in a liquid when the pressure of the gas increases?
According to Henry's law, what happens to the solubility of gas in a liquid when the pressure of the gas increases?
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In a solution where 34.2g of sugar are dissolved in 239.2g of syrup, what is the relevant calculation to find molarity?
In a solution where 34.2g of sugar are dissolved in 239.2g of syrup, what is the relevant calculation to find molarity?
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What indicates a positive deviation from Raoult's law?
What indicates a positive deviation from Raoult's law?
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Which of the following formulas correctly represents Raoult's law for a volatile solvent, A?
Which of the following formulas correctly represents Raoult's law for a volatile solvent, A?
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In the context of colligative properties, what does a decrease in vapor pressure of a solution compared to the pure solvent indicate?
In the context of colligative properties, what does a decrease in vapor pressure of a solution compared to the pure solvent indicate?
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What happens to the volume when a solution is mixed if AH is positive?
What happens to the volume when a solution is mixed if AH is positive?
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Which of the following describes an azeotropic mixture?
Which of the following describes an azeotropic mixture?
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What characterizes the relative lowering of vapor pressure?
What characterizes the relative lowering of vapor pressure?
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Which statement is true about maximum boiling point azeotropic mixtures?
Which statement is true about maximum boiling point azeotropic mixtures?
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What is the formula for the relative lowering of vapor pressure according to Raoult's law?
What is the formula for the relative lowering of vapor pressure according to Raoult's law?
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Study Notes
Chemical Kinetics
- Chemical Kinetics studies the rates of chemical reactions.
- Rate of reaction: The change in concentration of reactant or product per unit time.
- Elementary reaction: A reaction that occurs in a single step.
- Complex reaction: A reaction that occurs in more than one step.
- Rate laws describe the relationship between the rate of a reaction and the concentration of reactants.
- Order of reaction is determined experimentally, and represents the sum of the exponents of the concentration terms in the rate law.
- Rate constant (k) is a proportionality constant relating the rate of the reaction to the reactant concentrations.
- The units of the rate constant depend on the overall order of the reaction.
- Measuring reaction rates is important for understanding kinetics.
Rate of Reaction
- Rate of reaction is proportional to active masses of reactants raised to their stoichiometric coefficients.
- Rate law is determined experimentally.
- Rate = k[A]m[B]n
- k = rate constant
- m and n = orders with respect to A and B respectively
Zero Order Reaction
- Rate of reaction is independent of reactant concentrations.
- Rate = k
First Order Reaction
- Rate is directly proportional to the concentration of one reactant.
- Rate = k[A]
Half-life (t1/2)
- Time required for the concentration of a reactant to decrease to half its initial value.
- First Order: t1/2 = 0.693 / k
- Zero Order: t1/2 = [A]0 / 2k
Collision Theory
- Chemical reactions occur when reactant molecules collide with sufficient energy and proper orientation.
- Rate depends on: Collision frequency, Fraction of collisions with sufficient energy, Proper orientation of colliding molecules
Factors Affecting Reaction Rate
- Temperature: Increased temperature increases the rate.
- Concentration: Increased concentration increases the rate.
- Catalysts: Catalysts increase the rate without being consumed.
- Surface area: Increased surface area increases the rate (for heterogeneous reactions).
Arrhenius Equation
- Relates the rate constant (k) to temperature (T) and activation energy (Ea).
- k = Ae-Ea/RT
- A = pre-exponential factor
- R = ideal gas constant
Catalysts
- Substances that increase the rate of a reaction without being consumed.
- Provide an alternative reaction pathway with a lower activation energy.
Molecularity
- Total number of reactant molecules participating in a single step of a reaction.
- For elementary reactions, molecularity corresponds to order.
Solutions
- Homogeneous mixtures of two or more components.
- Components: Solute (dissolved substance) and solvent (the dissolving medium).
Concentration of Solution
- Molarity (M): Moles of solute per liter of solution.
- Molality (m): Moles of solute per kilogram of solvent.
- Mole fraction (X): The ratio of moles of a component to the total moles of solution.
Colligative Properties
- Properties of solutions that depend only on the number of solute particles, not on their identity.
- Examples: Vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure.
Colligative Properties: Vapor Pressure Lowering
- Vapor pressure of a solution is lower than the vapor pressure of the pure solvent.
- Vapor pressure lowering is directly proportional to the mole fraction of the solute.
- Ratio of vapor pressure of the solution to that of the pure solvent is equal to mole fraction of the solute,
Colligative Properties: Boiling Point Elevation
- Boiling point of a solution is higher than the boiling point of the pure solvent.
- Boiling point elevation is directly proportional to the molality of the solute.
Colligative Properties: Freezing Point Depression
- Freezing point of a solution is lower than the freezing point of the pure solvent.
- Freezing point depression is directly proportional to the molality of the solute.
Colligative Properties: Osmotic Pressure
- Osmotic pressure is the pressure required to prevent the flow of solvent across a semipermeable membrane.
- Osmotic pressure is directly proportional to the molarity of the solute.
- Increased concentration, higher osmotic pressure.
Electrochemistry
- The branch of chemistry that deals with the relationship between electricity and chemical reactions.
- Electrolytes: Substances that conduct electricity in solution or molten state.
- Non-electrolytes: Substances that do not conduct electricity in solution or molten state.
- Types of electrolytes: Strong and weak.
- Conductivity and Conductance: The ability of a solution to conduct electricity.
- Specific conductance (K): Conductance of a solution of 1cm length and 1 sq. cm cross-section area
- Molar Conductivity (∧m): Conductance of a solution in which the volume contains one mole of electrolyte.
- Kohlrausch's Law: At infinite dilution, the molar conductivity of an electrolyte is the sum of the ionic conductivities of the cation and the anion.
Electrolysis
- Electrochemical process where an electric current is passed through an ionic compound to cause a chemical reaction.
- Faraday's Laws: Relationship between amount of substance deposited/liberated at an electrode and quantity of charge passed.
- Electrolytic Cells: Cell in which electrolysis is carried out.
- Batteries: Electrochemical devices that convert chemical energy into electrical energy.
- Primary cells (non-rechargeable) and Secondary cells (rechargeable).
Electrode Potentials
- Potential difference between electrode and electrolyte.
- Standard Electrode Potential (E0): Electrode potential under standard conditions.
- Nernst Equation: Relates electrode potential to concentration of ion under nonstandard conditions.
Oxidation and Reduction
- Oxidation: Loss of electrons.
- Reduction: Gain of electrons.
- Redox reactions are coupled reactions, oxidation taking place at one electrode, and reduction at the other electrode.
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Description
Test your knowledge on chemical kinetics with this quiz covering reaction molecularity, rate laws, and the concepts of reaction order. Explore how changes in concentration affect the rate of a reaction and clarify common statements regarding reaction kinetics.
