Lecture 5: Spectroscopy and Photochemistry I
... break more and stronger bonds. We will pay special attention to them. ...
... break more and stronger bonds. We will pay special attention to them. ...
Cheat Sheet for Chemical Equilibrium
... subtracting “x” from reactants and adding “x” to products. • Given: Initial Concentrations of Products only‐ Reactants will be zero. Determine the change by subtracting “x” from the products and adding “x” to reactants. • Given: Initial Concentration of a species and Equilibrium concentration of ...
... subtracting “x” from reactants and adding “x” to products. • Given: Initial Concentrations of Products only‐ Reactants will be zero. Determine the change by subtracting “x” from the products and adding “x” to reactants. • Given: Initial Concentration of a species and Equilibrium concentration of ...
Name - Deans Community High School
... b) Is the forward reaction is exothermic or endothermic. ............................................ 1 c) Gold and platinum both catalyse the reaction. For the forward reaction EA using gold is 30 kJ, while EA using platinum is 40 kJ. i) using different dotted lines add this information to the grap ...
... b) Is the forward reaction is exothermic or endothermic. ............................................ 1 c) Gold and platinum both catalyse the reaction. For the forward reaction EA using gold is 30 kJ, while EA using platinum is 40 kJ. i) using different dotted lines add this information to the grap ...
Reaction Stoichiometry
... We cannot simply add the total moles of all the reactants to decide which reactant mixture makes the most product. We must always think about how much product can be formed by using what we are given, and the ratio in the balanced equation. ...
... We cannot simply add the total moles of all the reactants to decide which reactant mixture makes the most product. We must always think about how much product can be formed by using what we are given, and the ratio in the balanced equation. ...
Lecture 5 – Chemical Reactions
... They can be recognized because they have only one reactant, which breaks down to produce two or more products. ...
... They can be recognized because they have only one reactant, which breaks down to produce two or more products. ...
+ 2 HCL(aq) CaCl2(aq) + H2O(l) + CO2(g)
... Chemical Formula: States what elements a compound contains and the exact number of atoms of these elements. Oxidation Number: positive or negative number on the periodic table that indicates how many electrons an element has gained, lost or shared when bonding with another element. Polyatomic Atom: ...
... Chemical Formula: States what elements a compound contains and the exact number of atoms of these elements. Oxidation Number: positive or negative number on the periodic table that indicates how many electrons an element has gained, lost or shared when bonding with another element. Polyatomic Atom: ...
Chemistry 1. The Periodic Table displays the
... The enormous variety of biological, chemical, and physical properties of matter result from the ability of atoms to form bonds. This ability results from the electrostatic forces between electrons and protons and between atoms and molecules. As a basis for understanding this concept students know: a ...
... The enormous variety of biological, chemical, and physical properties of matter result from the ability of atoms to form bonds. This ability results from the electrostatic forces between electrons and protons and between atoms and molecules. As a basis for understanding this concept students know: a ...
Learning Outcomes
... and copper atoms. These exceptions are due to special stability associated with all the d orbitals being half filled or completely filled. When transition metals form ions it is the s electrons which are lost first rather than the d electrons. ...
... and copper atoms. These exceptions are due to special stability associated with all the d orbitals being half filled or completely filled. When transition metals form ions it is the s electrons which are lost first rather than the d electrons. ...
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.