Worksheet Key
... 36. For each system described below, indicate in which direction the equilibrium will shift when each stress is added or removed. Also explain how the system will react to alleviate the stress. a) N2 (g) + 3 H2 (g) 2 NH3 (g): more H2 is added to this reaction at equilibrium. Reaction will shift to ...
... 36. For each system described below, indicate in which direction the equilibrium will shift when each stress is added or removed. Also explain how the system will react to alleviate the stress. a) N2 (g) + 3 H2 (g) 2 NH3 (g): more H2 is added to this reaction at equilibrium. Reaction will shift to ...
AP CHEMISTRY - An Incomplete List of Topics
... IMF's - know the def and be able to identify the predominant IMF in a molecule ionic; network covalent; H-bond; dipole-dipole; LD, London Dispersion; IMF's and relation to bpt and m.pt Types of phase change Be able to label and read a heating/cooling curve and a phase diagram Know the def’s of boili ...
... IMF's - know the def and be able to identify the predominant IMF in a molecule ionic; network covalent; H-bond; dipole-dipole; LD, London Dispersion; IMF's and relation to bpt and m.pt Types of phase change Be able to label and read a heating/cooling curve and a phase diagram Know the def’s of boili ...
Fundamentals of Theoretical Organic Chemistry Lecture 1
... path is called an SN2 mechanism. In this case the reaction profile will look something like the one shown in Figure 1.1.1—3 In contrast to the above, if the bond breaking precedes the bond making, then only one molecule is involved; and therefore this nonsynchronous or stepwise path is called an SN1 ...
... path is called an SN2 mechanism. In this case the reaction profile will look something like the one shown in Figure 1.1.1—3 In contrast to the above, if the bond breaking precedes the bond making, then only one molecule is involved; and therefore this nonsynchronous or stepwise path is called an SN1 ...
Enthalpy
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
enthalpy of reaction
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
Thermo 2 - WordPress.com
... is changing in increments at which analysis can be done. If the time change at which the analysis is done is small enough, the system can be assumed to be in Quasi-equilibrium. • ALSO • For open systems (e.g. control volumes) the rate of change (mass flow) is assumed to be constant over a very short ...
... is changing in increments at which analysis can be done. If the time change at which the analysis is done is small enough, the system can be assumed to be in Quasi-equilibrium. • ALSO • For open systems (e.g. control volumes) the rate of change (mass flow) is assumed to be constant over a very short ...
Pictures and Graphs
... b) A solution is made using 70. g of potassium dichromate. Is the solution unsaturated, saturated, or supersaturated at 80oC? (highlight answer) c) A solution is made using 70. g of potassium nitrate. Is the solution unsaturated, saturated, or supersaturated at 80oC? (highlight answer) d) A solution ...
... b) A solution is made using 70. g of potassium dichromate. Is the solution unsaturated, saturated, or supersaturated at 80oC? (highlight answer) c) A solution is made using 70. g of potassium nitrate. Is the solution unsaturated, saturated, or supersaturated at 80oC? (highlight answer) d) A solution ...
2015-2016 AP CHEMISTRY MIDTERM EXAM Review
... 4. Answer all three portions in this part. Give the formulas to show the reactants and the products for the three following chemical reactions. Each reaction occurs in aqueous solution unless otherwise indicated. Represent the substances in solution as ions if the substance is extensively ionized. ...
... 4. Answer all three portions in this part. Give the formulas to show the reactants and the products for the three following chemical reactions. Each reaction occurs in aqueous solution unless otherwise indicated. Represent the substances in solution as ions if the substance is extensively ionized. ...
Chemistry Lesson Plans #07 - Chemical Reactions
... of Conservation of Mass? o In describing a chemical reaction you use statements such as Iron reacts with oxygen to produce iron(III) oxide which is called rust Or it could be written iron + oxygen iron(III) oxide • Note that the reactants are on the left of the arrow and the product is on the right ...
... of Conservation of Mass? o In describing a chemical reaction you use statements such as Iron reacts with oxygen to produce iron(III) oxide which is called rust Or it could be written iron + oxygen iron(III) oxide • Note that the reactants are on the left of the arrow and the product is on the right ...
Instrumental Methods of Analysis
... Principle: This technique involve the recording of difference in temperature between substance and reference material against time or temperature ,as the two specimens are subjected to identical temperature change in an environment heated or cooled at the controlled rate. Recording of results: DTA ...
... Principle: This technique involve the recording of difference in temperature between substance and reference material against time or temperature ,as the two specimens are subjected to identical temperature change in an environment heated or cooled at the controlled rate. Recording of results: DTA ...
Reactions
... 7. Always consult the Activity Series of metals and non-metals before attempting to write equations for replacement reactions. 8. If a reactant or product is solid, place (s) after the formula 9. If the reactant or product is a liquid, place (l) after the formula 10. If the reactant or product is a ...
... 7. Always consult the Activity Series of metals and non-metals before attempting to write equations for replacement reactions. 8. If a reactant or product is solid, place (s) after the formula 9. If the reactant or product is a liquid, place (l) after the formula 10. If the reactant or product is a ...
AP Chemistry: Chapter 13 Gaseous Equilibrium Section 1: Multiple
... (d) Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K. (e) For the reaction H2(g) + S2(g) H2S(g) at 483 K, calculate the value of the equilibrium constant, Kc. ...
... (d) Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K. (e) For the reaction H2(g) + S2(g) H2S(g) at 483 K, calculate the value of the equilibrium constant, Kc. ...
Answers to Homework Problem Sheet 11
... both doubled and this leads to the rate increasing by a factor of 16. As the reaction is first-order with respect to [H+], the rate would double because of the doubling in [H+]. The doubling in [Fe2+] therefore increases the rate by a factor of 8: the reaction is third-order (23 = 8) with respect to ...
... both doubled and this leads to the rate increasing by a factor of 16. As the reaction is first-order with respect to [H+], the rate would double because of the doubling in [H+]. The doubling in [Fe2+] therefore increases the rate by a factor of 8: the reaction is third-order (23 = 8) with respect to ...
computational chemistry
... The reader is advised to start with this book and to then delve further into the computational literature pertaining to his or her speci®c work. It is impossible to reference all relevant works in a book such as this. The bibliography included at the end of each chapter primarily lists textbooks and ...
... The reader is advised to start with this book and to then delve further into the computational literature pertaining to his or her speci®c work. It is impossible to reference all relevant works in a book such as this. The bibliography included at the end of each chapter primarily lists textbooks and ...
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.