Chemical kinetics

• Chemical kinetics


  The branch of chemistry concerned with the study of reaction rates, the factors that affect these rates, and the mechanisms by which reactions occur
• Chemical kinetics involves the investigation of how quickly reactants are converted into products in a chemical reaction and the pathways by which this transformation occurs
• Chemical kinetics


  • Understanding the factors influencing reaction rates, such as temperature, pressure, concentration of reactants, presence of catalysts, and nature of reactants
• Rate of a reaction


  Refers to how quickly reactants are converted into products in a chemical reaction
• Change in concentration


  The difference in the amount of a substance present at two different points in time
• Rate of reaction


  Typically expressed as the change in concentration of either a reactant or product over time
• The rate of a reaction can be affected by various factors
• Factors affecting the rate of reaction

  • Temperature
  • Concentration of reactants
  • Surface area
  • Presence of a catalyst
  • Nature of the reactants
• Rate of reaction

  • A[reactants]
• The rate equation is the mathematical expression that relates the reaction rate to the concentrations of reactants.

  
• Factors that affect the rate of reaction

  • Concentration of reactants
• Concentration of reactants decreases


  Rate of reaction increases
• Concentration of reactants increases


  Rate of reaction decreases
• Concentration of reactants increases


  The rate of reaction also increases
• Collision in chemistry


  Occurs when reactant particles collide with each other
• Reactant particles collide with each other


  They can either bounce off each other or react and form new products
• Delta


  Change in a variable
• Delta = 0.002 4/5
• Collision Theory fundamental concept in chemistry that explains by chemical reactions occur at the molecular level. It proposes that for a chemical reaction to take place, reactant molecules must collide with each other with sufficient energy and proper orientation
• Collision,reactant molecules must physically collid with each other to initiate a reaction. Not all collision results in a reaction,but collisions are a necessary for a reaction to occur
• Energy,the reacting molecules must have enough energy (kinetic energy) to overcome any activation energy barrier required for the formation of product molecules.
• Activation Energy amount of energy needed to start reaction, in order to speed up the reaction, catalysts are used. Enzymes are catalyst in cells
• Orientation,colliding particles must be oriented correctly so that they can interact effectively. This is called the correct geometry or configuration
• Increasing the temperature
• Higher temperatures


  Provide reactants with more kinetic energy
• More kinetic energy


  Leads to more frequent and energetic collisions
• More frequent and energetic collisions

  Increase the reaction rate
• Catalysts are substances that increase the rate of reaction by providing an alternative reaction pathway with a lower activation energy. Catalyst remain unchanged at the end of the reaction and can be used repeatedly
• The catalyst provides an alternate route which has a lower activation energy than the normal one.
• Cereal reactants


  • Have different reaction rates based on their chemical properties and molecular structures
  • Reactants with stronger bonds or higher stability may react faster compared to those with weaker bonds or lower stability
• Ionic compounds


  • React faster than covalent compounds
  • In reactions, bonds are broken and formed
  • When an ionic compound is placed in water, it dissociates
• Covalent bonds


  • It takes more energy to break covalent bonds
• Reactants with stronger bonds or higher stability


  May react more slowly because they require more energy to overcome the activation energy barrier and initiate the reaction. This higher energy requirement, along with fewer effective collisions, can lead to slower reaction rates compared to reactions involving weaker bonds or lower stability
• Metals


  • Are shiny, malleable, and good conductors of heat and electricity
  • Typically found on the left and middle of the periodic table
  • Have properties intermediate between metals and nonmetals, exhibiting varying degrees of conductivity and brittleness
  • Are located to the right of hydrogen
• Ionic compounds


  • Formed by the complete transfer of electrons
  • Exist in a solid-state
  • Good conductors of electricity in the molten state as well as in aqueous solutions
  • Soluble in water
• Covalent compounds


  • Formed by the sharing of electrons between two atoms
  • Exist in all three states: solid, liquid, gas
  • Have high melting and boiling points
  • Generally insoluble in water
  • Are insulators as they do not conduct electricity in the molten state as well as in aqueous solutions
• Reactants have different reaction rates based on the chemical properties and molecular structures
• Ionic compounds are formed by the complete transfer of electrons and exist in a solid-state. They are good conductors of electricity in the molten state as well as in aqueous solutions and are soluble in water