Basic Physical Chemistry 3
... applications of the first and second laws to chemical and physical changes. Applications are made to chemical equilibrium, electrochemical cells, and other spontaneous processes. Course Objectives: Upon successful completion of this course the student should be able to: 1. Apply physical chemistry p ...
... applications of the first and second laws to chemical and physical changes. Applications are made to chemical equilibrium, electrochemical cells, and other spontaneous processes. Course Objectives: Upon successful completion of this course the student should be able to: 1. Apply physical chemistry p ...
Gas and Thermo Notes
... container. All collisions are perfectly elastic. The average kinetic energy for molecules is the same for all gases at the same temperature, and its value is directly proportional to the absolute temperature. ...
... container. All collisions are perfectly elastic. The average kinetic energy for molecules is the same for all gases at the same temperature, and its value is directly proportional to the absolute temperature. ...
File
... Describe and write a balanced chemical equation (including proper labels for solids, liquids, gases, and aqueous solutions). Describe, identify, and predict the products of the five general types of reactions (synthesis, decomposition, single replacement, double replacement, and combustion) Explain ...
... Describe and write a balanced chemical equation (including proper labels for solids, liquids, gases, and aqueous solutions). Describe, identify, and predict the products of the five general types of reactions (synthesis, decomposition, single replacement, double replacement, and combustion) Explain ...
Inquiry: Calculation - Coristines
... 1. Explain the difference between heat capacity, thermal energy, specific heat capacity, enthalpy and molar enthalpy. (5 marks) 2. a) Explain the three types of molecular motion as a result of kinetic energy (3marks) b) Why does neon have a lower molar heat capacity than nitrogen ? (2 mark) C) When ...
... 1. Explain the difference between heat capacity, thermal energy, specific heat capacity, enthalpy and molar enthalpy. (5 marks) 2. a) Explain the three types of molecular motion as a result of kinetic energy (3marks) b) Why does neon have a lower molar heat capacity than nitrogen ? (2 mark) C) When ...
Periodic Table, Bonding, Reactions, and Moles
... 13. Identify the two types of bonds in the compound sodium stearate. Base your answers to questions 14 through 16 on the information below. The Solvay process is a multistep industrial process used to produce washing soda, Na2CO3 (s). In the last step of the Solvay process, NaHCO3 (s) is heated to 3 ...
... 13. Identify the two types of bonds in the compound sodium stearate. Base your answers to questions 14 through 16 on the information below. The Solvay process is a multistep industrial process used to produce washing soda, Na2CO3 (s). In the last step of the Solvay process, NaHCO3 (s) is heated to 3 ...
1. This is a question about trends in chemistry In
... Using the information above, calculate the pre-exponential factor, A, and the activation energy for the dimerization of 1,3-butadiene. Your answers must include the appropriate units. ...
... Using the information above, calculate the pre-exponential factor, A, and the activation energy for the dimerization of 1,3-butadiene. Your answers must include the appropriate units. ...
Student Exploration Sheet: Growing Plants
... new substances. The substances that undergo change are called reactants. The new substances are products. Sometimes during a chemical reaction, one type of reactant will be used up before the other reactants. This reactant is the limiting reactant. Using the Limiting Reactants Gizmo™, you can determ ...
... new substances. The substances that undergo change are called reactants. The new substances are products. Sometimes during a chemical reaction, one type of reactant will be used up before the other reactants. This reactant is the limiting reactant. Using the Limiting Reactants Gizmo™, you can determ ...
A matter of Equilibrium
... Such reactions are called irreversible However many reactions can proceed in either direction: If we mix pure N2 and H2 we form ammonia: N2 (g) + 3 H2 (g) → 2 NH3 (g) But if we take pure ammonia we form N2 and H2: 2 NH3 (g) → N2 (g) + 3 H2 (g) Such reactions are called reversible ...
... Such reactions are called irreversible However many reactions can proceed in either direction: If we mix pure N2 and H2 we form ammonia: N2 (g) + 3 H2 (g) → 2 NH3 (g) But if we take pure ammonia we form N2 and H2: 2 NH3 (g) → N2 (g) + 3 H2 (g) Such reactions are called reversible ...
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.