Chemistry- CST Review
... 2. What factors increase the rate (speed) of a reaction? (Like concentration, pressure, and temperature) The increase of concentration of reactants, pressure, and temperature are factors that increase reaction rate. 3. What does a catalyst do to the reaction rate? A catalyst decreases the activation ...
... 2. What factors increase the rate (speed) of a reaction? (Like concentration, pressure, and temperature) The increase of concentration of reactants, pressure, and temperature are factors that increase reaction rate. 3. What does a catalyst do to the reaction rate? A catalyst decreases the activation ...
Topic 1: Quantitative Chemistry
... 1.3.2 Identify the mole ratio of any two species in a chemical equation. 1.3.3 Apply the state symbols (s), (l), (g), and (aq). 1.4 Mass and gaseous volume relationships in chemical reactions 1.4.1 Calculate theoretical yields from chemical equations. 1.4.2 Determine the limiting reactant and the re ...
... 1.3.2 Identify the mole ratio of any two species in a chemical equation. 1.3.3 Apply the state symbols (s), (l), (g), and (aq). 1.4 Mass and gaseous volume relationships in chemical reactions 1.4.1 Calculate theoretical yields from chemical equations. 1.4.2 Determine the limiting reactant and the re ...
Name: ______ Date
... a) A process that absorbs energy from its surroundings is called endothermic. b) In an exothermic reaction the enthalpy of species increases. c) Energy is the capacity to do work or to transfer heat. d) Kinetic energy is the energy of motion. There are two properties of a reacting system that determ ...
... a) A process that absorbs energy from its surroundings is called endothermic. b) In an exothermic reaction the enthalpy of species increases. c) Energy is the capacity to do work or to transfer heat. d) Kinetic energy is the energy of motion. There are two properties of a reacting system that determ ...
Description: This is an advanced placement course designed to
... 2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry 3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes 4. Relationship of change in ...
... 2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry 3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes 4. Relationship of change in ...
Branches of Chemistry
... According to this law, the total mass of the products of a chemical reaction is equal to the total mass of the substances that react together. Law of constant composition – No matter how a substance is made, it will always contain the same elements in the same proportions. [Joseph Proust, 1779] By P ...
... According to this law, the total mass of the products of a chemical reaction is equal to the total mass of the substances that react together. Law of constant composition – No matter how a substance is made, it will always contain the same elements in the same proportions. [Joseph Proust, 1779] By P ...
CHE 1401 - Spring 2015 - Chapter 5 Homework 5 (Chapter 5
... B) H is the value of q measured under conditions of constant volume. C) The enthalphy change for a reaction is independent of the state of the reactants and products. D) Enthalpy is a state function. E) Enthalpy is an intensive property. ...
... B) H is the value of q measured under conditions of constant volume. C) The enthalphy change for a reaction is independent of the state of the reactants and products. D) Enthalpy is a state function. E) Enthalpy is an intensive property. ...
CHE 1401 - Fall 2015 - Chapter 5 Homework 5 (Chapter 5
... MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1°F. There are _________ ...
... MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1°F. There are _________ ...
CHE 1401 - Fall 2016 - Chapter 5 Homework 5 (Chapter 5
... is __________, and therefore heat is __________ by the reaction. A) exothermic, absorbed B) exothermic, released C) endothermic, released D) endothermic, absorbed E) thermoneutral, neither released nor absorbed 27) Which of the following is a statement of Hess's law? A) The ΔH for a process in the f ...
... is __________, and therefore heat is __________ by the reaction. A) exothermic, absorbed B) exothermic, released C) endothermic, released D) endothermic, absorbed E) thermoneutral, neither released nor absorbed 27) Which of the following is a statement of Hess's law? A) The ΔH for a process in the f ...
CHE 1401 - Spring 2016 - Chapter 5 Homework 5 (Chapter 5
... is __________, and therefore heat is __________ by the reaction. A) exothermic, released B) exothermic, absorbed C) endothermic, released D) endothermic, absorbed E) thermoneutral, neither released nor absorbed 9) Of the following, which one is a state function? A) q B) w C) heat D) H E) none of the ...
... is __________, and therefore heat is __________ by the reaction. A) exothermic, released B) exothermic, absorbed C) endothermic, released D) endothermic, absorbed E) thermoneutral, neither released nor absorbed 9) Of the following, which one is a state function? A) q B) w C) heat D) H E) none of the ...
AP Chem Test 5-7 Practice Exam - mvhs
... the alkaline earth element with the smallest atomic radius the element with the largest ionization energy in Group 5A the element whose 2+ ion has the configuration [Kr] 4d5 the element with the most negative electron affinity in Group 7A the element whose electron configuration is [Ar]3d104s2 ...
... the alkaline earth element with the smallest atomic radius the element with the largest ionization energy in Group 5A the element whose 2+ ion has the configuration [Kr] 4d5 the element with the most negative electron affinity in Group 7A the element whose electron configuration is [Ar]3d104s2 ...
CHEM1405 2012-J-2 June 2012 • What is the ground state electron
... Why is ΔG not equal to ΔH for this reaction? By definition, ΔG = ΔH – TΔS. As the entropy change for the reaction and the temperature are not zero, so ΔG ≠ ΔH. The pH of pure water is 6.81 at 37 °C. Is water acidic, basic or neutral at this temperature? Explain. Neutral. Pure water is neutral at all ...
... Why is ΔG not equal to ΔH for this reaction? By definition, ΔG = ΔH – TΔS. As the entropy change for the reaction and the temperature are not zero, so ΔG ≠ ΔH. The pH of pure water is 6.81 at 37 °C. Is water acidic, basic or neutral at this temperature? Explain. Neutral. Pure water is neutral at all ...
sample - Bright Red Publishing
... the enthalpy of a substance. Only values relative to an arbitrary reference point can be given and for all enthalpy expressions, this reference point is called the standard enthalpy of formation. The standard enthalpy of formation (∆H°f ) is defined as the enthalpy change involved when one mole of a ...
... the enthalpy of a substance. Only values relative to an arbitrary reference point can be given and for all enthalpy expressions, this reference point is called the standard enthalpy of formation. The standard enthalpy of formation (∆H°f ) is defined as the enthalpy change involved when one mole of a ...
AS specification - word format File
... a demonstrate an understanding of the term enthalpy change, ΔH b construct simple enthalpy level diagrams showing the enthalpy change c recall the sign of ΔH for exothermic and endothermic reactions, eg illustrated by the use of exo- and endothermic reactions in hot and cold packs d recall the defin ...
... a demonstrate an understanding of the term enthalpy change, ΔH b construct simple enthalpy level diagrams showing the enthalpy change c recall the sign of ΔH for exothermic and endothermic reactions, eg illustrated by the use of exo- and endothermic reactions in hot and cold packs d recall the defin ...
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.