South Pasadena • AP Chemistry
... The chemical elements are the building blocks of matter, which can be understood in terms of arrangements of atoms. Molecules & elements Chemical analysis The mole Electron configuration Periodicity Quantum mechanical model Atomic models Mass spectrometry Light & matter Conservat ...
... The chemical elements are the building blocks of matter, which can be understood in terms of arrangements of atoms. Molecules & elements Chemical analysis The mole Electron configuration Periodicity Quantum mechanical model Atomic models Mass spectrometry Light & matter Conservat ...
Notes on Chapter 12 Chemical Equilibrium
... Factors that affect the rate of reaction: a. temperature- increase in temperature increases reaction rates b. concentration- increase in the concentration of reactant(s) increases rates c. catalyst = anything that speeds up the rate of reactions by lowering the energy of activation for the reaction. ...
... Factors that affect the rate of reaction: a. temperature- increase in temperature increases reaction rates b. concentration- increase in the concentration of reactant(s) increases rates c. catalyst = anything that speeds up the rate of reactions by lowering the energy of activation for the reaction. ...
Equilibrium - Cobb Learning
... Strike a match and it erupts instantaneously. Coal made from dead plants takes millions of years ...
... Strike a match and it erupts instantaneously. Coal made from dead plants takes millions of years ...
Equilibrium and Kinetics
... 9. The half-life of a first order reaction is 24 days. (i) Calculate the rate constant for the reaction (ii) The time taken for 75% of the reactant to decay. 10. Derive an expression for the variation of reactant concentration with respect to time for a reaction which exhibits zero order kinetics. H ...
... 9. The half-life of a first order reaction is 24 days. (i) Calculate the rate constant for the reaction (ii) The time taken for 75% of the reactant to decay. 10. Derive an expression for the variation of reactant concentration with respect to time for a reaction which exhibits zero order kinetics. H ...
Collision Theory
... Theories of Chemical Kinetics: Collision Theory • Before atoms/molecules/ions can react, they must first collide • An effective collision between two species puts enough energy to break key bonds • The activation energy (Ea) is the minimum energy that must be supplied by collisions to trigger a rea ...
... Theories of Chemical Kinetics: Collision Theory • Before atoms/molecules/ions can react, they must first collide • An effective collision between two species puts enough energy to break key bonds • The activation energy (Ea) is the minimum energy that must be supplied by collisions to trigger a rea ...
CHM 111: General Physical Chemistry 3 Units
... real gases and deviations from ideal gas laws; liquid, macroscopic properties of liquids, evaporation, vapor pressure and its variation with temperature, boiling point, heat of vaporization, Clausius-Clapeyron equation, freezing point, melting point and phase diagrams of simple systems; solids types ...
... real gases and deviations from ideal gas laws; liquid, macroscopic properties of liquids, evaporation, vapor pressure and its variation with temperature, boiling point, heat of vaporization, Clausius-Clapeyron equation, freezing point, melting point and phase diagrams of simple systems; solids types ...
Transition state theory
Transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes.TST is used primarily to understand qualitatively how chemical reactions take place. TST has been less successful in its original goal of calculating absolute reaction rate constants because the calculation of absolute reaction rates requires precise knowledge of potential energy surfaces, but it has been successful in calculating the standard enthalpy of activation (Δ‡Hɵ), the standard entropy of activation (Δ‡Sɵ), and the standard Gibbs energy of activation (Δ‡Gɵ) for a particular reaction if its rate constant has been experimentally determined. (The ‡ notation refers to the value of interest at the transition state.)This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as ""activated-complex theory,"" ""absolute-rate theory,"" and ""theory of absolute reaction rates.""Before the development of TST, the Arrhenius rate law was widely used to determine energies for the reaction barrier. The Arrhenius equation derives from empirical observations and ignores any mechanistic considerations, such as whether one or more reactive intermediates are involved in the conversion of a reactant to a product. Therefore, further development was necessary to understand the two parameters associated with this law, the pre-exponential factor (A) and the activation energy (Ea). TST, which led to the Eyring equation, successfully addresses these two issues; however, 46 years elapsed between the publication of the Arrhenius rate law, in 1889, and the Eyring equation derived from TST, in 1935. During that period, many scientists and researchers contributed significantly to the development of the theory.