Presentation on theme: "KINETICS How Fast Does A Reaction Occur? Energy Diagrams l Reactants always start a reaction so they are on the left side of the diagram. Reactants l."— Presentation transcript:
l In an endothermic graph, the products have greater energy than the reactants. Reactants l The change in energy is a positive value. Products
Exothermic And Endothermic Reactions l Scientists have observed that the energy released in the formation of a compound from its elements is always identical to the energy required to decompose that compound into its elements.
Energy Diagrams l Activation energy is the minimum amount of energy that reacting particles must have to form the activated complex. Activation energy activated complex
Energy Diagrams l The activated complex is a short- lived, unstable arrangement of atoms that may break apart and re- form the reactants or may form products. activated complex
Energy Diagrams l To calculate the activation energy, subtract the energy of the reactants from the energy at the top of the peak. Activation energy
Energy Diagrams The enthalpy or heat of reaction ( Δ H) is the amount of heat released or absorbed in the reaction. Enthalpy/heat of reaction ( Δ H)
Energy Diagrams To determine Δ H, take the energy of the products and subtract the energy of the reactants. Enthalpy/heat of reaction ( Δ H)
Problem l The heat content of the reactants of the forward reaction is about ______ kilojoules. (80 kJ)
Problem l The heat content of the products of the forward reaction is about ______ kilojoules. (160 kJ)
Problem l The heat content of the activated complex of the forward reaction is about _____ kilojoules. (240 kJ)
Problem l The activation energy of the forward reaction is about _____ kilojoules. (160 kJ)
Problem The heat of reaction ( Δ H) of the forward reaction is about _____ kilojoules. (80 kJ)
Problem l The forward reaction is (endothermic or exothermic). (endothermic - products are higher in energy)
Problem l The activation energy of the reverse reaction is about _____ kilojoules. (80 kJ)
Problem The heat of reaction ( Δ H) of the reverse reaction is about _____ kilojoules. (- 80 kJ)
Problem l The reverse reaction is (endothermic or exothermic). (exothermic - products are lower in energy)
Energy Diagrams l The activation energy can be lowered by adding a catalyst. effect of the catalyst
Energy Diagrams l The catalyst lowers the activation energy by providing an alternate pathway for the reaction to occur. effect of the catalyst
Collision Theory l According to the collision theory, atoms, ions, and molecules must collide with each other in order to react.
Collision Theory l The following three statements summarize the collision theory. 1. Particles must collide in order to react. 2. The particles must collide with the correct orientation.
Collision Theory 3. The particles must collide with enough energy to form an unstable activated complex, also called a transition state, which is an intermediate particle made up of the joined reactants.
Collision Theory l The minimum amount of energy that colliding particles must have in order to form an activated complex is called the activation energy of the reaction. l Particles that collide with less energy than the activation energy cannot form an activated complex.
Collision Theory l In an exothermic reaction, molecules collide with enough energy to overcome the activation energy barrier, form an activated complex, then release energy and form products at a lower energy level.
Energy Reaction coordinate Reactants Products Activated Complex or Transition State
Energy Reaction coordinate Reactants Products Activation Energy
Energy Reaction coordinate Reactants Products Overall energy change
Collision Theory l In the reverse endothermic reaction, the reactant molecules lying at a low energy level must absorb energy to overcome the activation energy barrier and form high-energy products.
Factors Affecting Reaction Rates l The reaction rate for almost any chemical reaction can be modified by varying the conditions of the reaction.
Factors Affecting Reaction Rates 1)An important factor that affects the rate of a chemical reaction is the reactive nature of the reactants. As you know, some substances react more readily than others. The more reactive a substance is, the faster the reaction rate.
Factors Affecting Reaction Rates 2)Another important factor that affects the rate of a chemical reaction is the concentration of the reactants. Reactions speed up when the concentrations of reacting particles are increased. Increasing the number of reactants increases probability of collisions.
Factors Affecting Reaction Rates 2)continued. The rate of gaseous reactions can be increased by pumping more gas into the reaction container.
Factors Affecting Reaction Rates 3)Surface area of the reactants affects the rate of a chemical reaction. Increasing the surface area of reactants provides more opportunity for collisions with other reactants, thereby increasing the reaction rate.
Factors Affecting Reaction Rates 4)Temperature affects the rate of a chemical reaction. Generally, increasing the temperature at which a reaction occurs increases the reaction rate. Raising the temperature raises both the collision frequency and the collision energy.
Factors Affecting Reaction Rates 5)Adding a catalyst affects the rate of a chemical reaction. A catalyst is a substance that increases the rate of a chemical reaction without itself being consumed in the reaction. In fact, catalysts are not included in the chemical equation.
Factors Affecting Reaction Rates A catalyst lowers the activation energy of a reaction by providing an alternate pathway for the reaction to occur (the blue line).