Rates of Reaction
Rates of Reaction
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Reaction kinetics
Reaction kinetics
The study of the rates of chemical reactions
The study of the rates of chemical reactions
The rate of reaction can be defined as:
Rate = Change in amount of reactant and product/time
Collision theory
Collision theory
Collision theory states that when suitable particles of the reactant hit each other, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The minimum energy that colliding particle mist posses for a successful collision to take place is called the activation energy
Collision theory states that when suitable particles of the reactant hit each other, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The minimum energy that colliding particle mist posses for a successful collision to take place is called the activation energy
Exothermic
Exothermic
Endothermic
Endothermic
Effects of variables on the rate of reaction
Effects of variables on the rate of reaction
Concentration
Concentration
If you increase the concentration of a reactant, there will be more of the chemical present. More reactant particles moving together allow more collisions to happen and so the reaction rate is increased. The higher the concentration of reactants, the faster the rate of a reaction will be.
If you increase the concentration of a reactant, there will be more of the chemical present. More reactant particles moving together allow more collisions to happen and so the reaction rate is increased. The higher the concentration of reactants, the faster the rate of a reaction will be.
Temperature
Temperature
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision
Boltzmann distribution
Boltzmann distribution
A Boltzmann Distribution shows the distribution of molecular energies in a gas at constant temperature. Most gas molecules have energies within a comparatively narrow range. The curve will only meet the energy axis at infinity energy. The area under the curve gives the total number of gas molecules. Therefore, increasing the temperature increases the rate of reaction because:
A Boltzmann Distribution shows the distribution of molecular energies in a gas at constant temperature. Most gas molecules have energies within a comparatively narrow range. The curve will only meet the energy axis at infinity energy. The area under the curve gives the total number of gas molecules. Therefore, increasing the temperature increases the rate of reaction because:
Catalyst
Catalyst
Homogenous
Homogenous
Homogeneous catalysts are those which exist in the same phase (gas or liquid) as the reactants, while heterogeneous catalysts are not in the same phase as the reactants. Typically, heterogeneous catalysis involves the use of solid catalysts placed in a liquid reaction mixture.
Homogeneous catalysts are those which exist in the same phase (gas or liquid) as the reactants, while heterogeneous catalysts are not in the same phase as the reactants. Typically, heterogeneous catalysis involves the use of solid catalysts placed in a liquid reaction mixture.
Heterogenous
Heterogenous
heterogeneous catalysis is catalysis where the phase of catalysts differs from that of the reactants or products. The process contrasts with homogeneous catalysis where the reactants, products and catalyst exist in the same phase.
heterogeneous catalysis is catalysis where the phase of catalysts differs from that of the reactants or products. The process contrasts with homogeneous catalysis where the reactants, products and catalyst exist in the same phase.
Enzymes
Enzymes
Enzymes are catalysts that drive reaction rates forward. Most catalysts, but not all, are made up of amino acid chains called proteins that accelerate the rate of reactions in chemical systems.
Enzymes are catalysts that drive reaction rates forward. Most catalysts, but not all, are made up of amino acid chains called proteins that accelerate the rate of reactions in chemical systems.
Videos
Videos
Maxwell Boltzmann distribution curve
Maxwell Boltzmann distribution curve
Rate of reaction
Rate of reaction
Rate of reaction
Rate of reaction
Haber and contact process
Haber and contact process
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