Lecture 01

• What is the main difference between kinetics and thermodynamics?

  Kinetics studies reaction rates, thermodynamics studies feasibility
• What factors determine the kinetics of a chemical reaction?

  Nature of reactants, temperature, concentration, surface area
• What is the concept of reaction rate?

  Speed at which reactants convert to products
• How can you determine the units for different reaction rates?

  By analysing changes in concentration over time
• What does a negative ΔG indicate about a reaction?

  The reaction is spontaneous but not necessarily fast
• What does thermodynamics study in relation to chemical reactions?

  Feasibility of reactions from an energetic perspective
• What does kinetics study in relation to chemical reactions?

  How fast reactions occur
• Can thermodynamically favorable reactions occur slowly?

  Yes, due to slow kinetics
• What occurs during a chemical reaction?

  Bonds in reactants break and new bonds form
• How do the state of matter and intermolecular interactions affect reaction rates?

  They influence the speed of molecular collisions
• What is required for a chemical reaction to occur?

  Efficient collisions between reactants

  
• How do bond types affect reaction rates?

  Bond strength and polarity influence reaction speed
• Why do triple bonds affect reaction rates?

  They are harder to break than single bonds
• How do ionic substances compare to covalent substances in terms of reaction rates?

  Ionic substances react faster due to efficient electron rearrangement

  
• What determines the reactivity of single-atom substances?

  Electron shell structure and bonding strength
• How does molecular shape affect reaction rates?

  Complex shapes can hinder effective collisions
• What role does temperature play in reaction rates?

  Higher temperatures increase reaction rates
• How does concentration affect reaction rates?

  Higher concentration increases the probability of collisions
• What is the Le-Chatelier Principle?

  System shifts to restore equilibrium after disturbance
• How does surface area affect reaction rates?

  Larger surface areas increase collision opportunities
• What is the effect of catalysts on reaction rates?

  Catalysts lower activation energy and increase rates
• What is the difference between catalysts and inhibitors?

  Catalysts increase rates, inhibitors decrease rates
• How are reaction rates monitored and measured?

  By changes in concentration of reactants or products

  
• What sign indicates reactants are consumed in a reaction rate expression?

  Negative sign for reactants' concentrations
• What sign indicates products are formed in a reaction rate expression?

  Positive sign for products' concentrations
• What do [A] and [B] represent in reaction rate expressions?

  Concentrations of reactants
• What are reaction orders in relation to reaction rates?

  Empirical values based on experimental data
• How is the total order of a reaction calculated?

  By summing the exponents of reactants
• What is molecularity in a reaction?

  Number of molecules in the rate-determining step
• What is a unimolecular reaction?

  Involves only one molecule undergoing a reaction
• What is a bimolecular reaction?

  Involves the collision of two molecules
• What is a multimolecular reaction?

  Involves the simultaneous collision of three molecules
• What characterizes zero-order reactions?

  Rate is independent of reactant concentration
• What characterises first-order reactions?

  Rate depends on the concentration of one reactant
• What characterises second-order reactions?

  Rate is proportional to the square of concentration
• How does the rate of reaction change with increased surface area?

  Increased surface area leads to faster reaction rates
• What happens to reaction rates when solids are crushed?

  Crushed solids increase surface area and reaction rates
• What is the effect of viscosity on reaction rates?

  More viscous solvents slow down reaction rates
• What is the relationship between temperature and kinetic energy of molecules?

  Higher temperature increases kinetic energy of molecules
• How does temperature affect the flexibility of molecules?

  Increased temperature results in greater molecular flexibility