K c
... experimental conditions may disturb the balance and shift the equilibrium position so that more or less of the desired product is formed. • In this section we will study 5 factor which can effect chemical equilibrium namely : concentration, pressure, volume, temperature, and catalyst. • Le Châtelier ...
... experimental conditions may disturb the balance and shift the equilibrium position so that more or less of the desired product is formed. • In this section we will study 5 factor which can effect chemical equilibrium namely : concentration, pressure, volume, temperature, and catalyst. • Le Châtelier ...
H2 Chemistry Syllabus (9729)
... concept that the four valence bonds of a carbon atom are oriented in a tetrahedral configuration, which led to the development of the stereochemical concept. This has important applications, particularly in the pharmaceutical industry as many drugs are active only in one particular enantiomeric form ...
... concept that the four valence bonds of a carbon atom are oriented in a tetrahedral configuration, which led to the development of the stereochemical concept. This has important applications, particularly in the pharmaceutical industry as many drugs are active only in one particular enantiomeric form ...
Various Types of RXNS
... 5. small chunks of solid sodium are added to water --describe a test to confirm the gaseous product in your reaction 6. hydrobromic acid is added to a solution of potassium hydrogen carbonate --when a gas produced by the reaction is bubbled through limewater, what visible change is expected? 7. aque ...
... 5. small chunks of solid sodium are added to water --describe a test to confirm the gaseous product in your reaction 6. hydrobromic acid is added to a solution of potassium hydrogen carbonate --when a gas produced by the reaction is bubbled through limewater, what visible change is expected? 7. aque ...
Low sticking probability in the nonactivated dissociation of N2
... molecular adsorption takes place. Measurements of the initial sticking coefficient S0 as a function of the N2 initial kinetic energy Ei show that S0 is nearly constant 共⬃10−3兲 for low Ei, then increases rather quickly in the range of 0.4 ⬍ Ei ⬍ 1.2 eV and levels off at higher Ei.6 This S-type curve, ...
... molecular adsorption takes place. Measurements of the initial sticking coefficient S0 as a function of the N2 initial kinetic energy Ei show that S0 is nearly constant 共⬃10−3兲 for low Ei, then increases rather quickly in the range of 0.4 ⬍ Ei ⬍ 1.2 eV and levels off at higher Ei.6 This S-type curve, ...
materials required/recommended for this paper
... that square then shade your new answer. Do not erase or use correction fluid/tape. Marks will not be deducted for incorrect answers. No marks will be given if more than one answer is completed for any question. Sections Two and Three: Write your answers in this Question/Answer Booklet. ...
... that square then shade your new answer. Do not erase or use correction fluid/tape. Marks will not be deducted for incorrect answers. No marks will be given if more than one answer is completed for any question. Sections Two and Three: Write your answers in this Question/Answer Booklet. ...
PowerPoint Presentation - Chemical Equilibrium
... The point where the two curves cross shows the concentrations of reactants and products at equilibrium. The slopes of tangent lines to each curve at a specific time prior to reaching equilibrium are equal, but opposite, because the stoichiometry between the products and reactants is all 1:1. Equilib ...
... The point where the two curves cross shows the concentrations of reactants and products at equilibrium. The slopes of tangent lines to each curve at a specific time prior to reaching equilibrium are equal, but opposite, because the stoichiometry between the products and reactants is all 1:1. Equilib ...
CHEMISTRY 102A/102C Spring 2014 Hour Exam II Page _____ For
... II. Non-ideal gas behavior is the result of the real volume of gas particles and the intermolecular attractions between gas particles. III. The effect of attractive forces between gas particles can be reduced by heating the gas. IV. 1.00 1023 gas molecules placed in a closed 5.0 liter container at ...
... II. Non-ideal gas behavior is the result of the real volume of gas particles and the intermolecular attractions between gas particles. III. The effect of attractive forces between gas particles can be reduced by heating the gas. IV. 1.00 1023 gas molecules placed in a closed 5.0 liter container at ...
Topic 7.2 Equilibrium The Position of Equilibrium
... If the equilibrium concentrations are as follows: [CO] = 1.00 M, [H2O] = 0.025, [CO2] = 0.075 M and [H2] = 0.060 M, calculate the equilibrium constant. ...
... If the equilibrium concentrations are as follows: [CO] = 1.00 M, [H2O] = 0.025, [CO2] = 0.075 M and [H2] = 0.060 M, calculate the equilibrium constant. ...
BH - hrsbstaff.ednet.ns.ca
... solution is the limit to the amount of solute that can dissolve into a solvent. If there is more than the saturation point then it is called supersaturated and if there is less solute than the saturation point it is called unsaturated. The temperature of a solution changes the saturation point of th ...
... solution is the limit to the amount of solute that can dissolve into a solvent. If there is more than the saturation point then it is called supersaturated and if there is less solute than the saturation point it is called unsaturated. The temperature of a solution changes the saturation point of th ...
Chapter 19 Chemical Thermodynamics
... • Boltzmann envisioned the motions of a sample of molecules at a particular instant in time. This would be akin to taking a snapshot of all the molecules. ...
... • Boltzmann envisioned the motions of a sample of molecules at a particular instant in time. This would be akin to taking a snapshot of all the molecules. ...
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.