402 - Sydenham High School
... I now understand the difference between a strong and weak acid and a strong and weak base. Now I have to remember to distinguish between strength and concentration. This takes mental effort The fact that sometimes a chemical can act as an acid in one reaction and as a base in another reaction is int ...
... I now understand the difference between a strong and weak acid and a strong and weak base. Now I have to remember to distinguish between strength and concentration. This takes mental effort The fact that sometimes a chemical can act as an acid in one reaction and as a base in another reaction is int ...
Chapter 8powerp point for chemical reactions
... A list of elements organized according to the ease with which the elements undergo certain chemical reactions Used to help predict whether certain chemical reactions will occur ...
... A list of elements organized according to the ease with which the elements undergo certain chemical reactions Used to help predict whether certain chemical reactions will occur ...
Equilibrium (Sheet 1)
... H2 + CO2 + heat. If no stress is introduced into this system, then the concentration of H 2O, CO, H2, and CO2 will not change. Now then, assume the concentration of H2O was increased, then effectively the number of collisions between H2O molecules and CO molecules are increased, resulting in an incr ...
... H2 + CO2 + heat. If no stress is introduced into this system, then the concentration of H 2O, CO, H2, and CO2 will not change. Now then, assume the concentration of H2O was increased, then effectively the number of collisions between H2O molecules and CO molecules are increased, resulting in an incr ...
Name: 1) In a chemical reaction, the difference between the
... Given the system at equilibrium: N2 O4 (g) + 58.1 kJ ‰Š‹ 2NO2 (g) What will be the result of an increase in temperature at constant pressure? A) The equilibrium will shift to the left, and the concentration of NO2 (g) will decrease. B) The equilibrium will shift to the left, and the concentration of ...
... Given the system at equilibrium: N2 O4 (g) + 58.1 kJ ‰Š‹ 2NO2 (g) What will be the result of an increase in temperature at constant pressure? A) The equilibrium will shift to the left, and the concentration of NO2 (g) will decrease. B) The equilibrium will shift to the left, and the concentration of ...
Test 9 Review - Evan`s Chemistry Corner
... Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions. An effective collision is one in which the colliding particles approach each other at the proper angle and with the proper amount of energy to cause a reaction. The greater ...
... Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions. An effective collision is one in which the colliding particles approach each other at the proper angle and with the proper amount of energy to cause a reaction. The greater ...
The first law of thermodynamics
... and potential energy, explain the definitions and the each of deriving procedure. ...
... and potential energy, explain the definitions and the each of deriving procedure. ...
Types of Chemical Reactions
... There are many types of chemical reactions. Five of the most common are: synthesis: two or more reactants combine to form a single product. A+BC decomposition: one reactant disintegrates (decomposes) to form two or more products: AB+C single replacement (sometimes called single displacement): atom ...
... There are many types of chemical reactions. Five of the most common are: synthesis: two or more reactants combine to form a single product. A+BC decomposition: one reactant disintegrates (decomposes) to form two or more products: AB+C single replacement (sometimes called single displacement): atom ...
Factors Affecting the Rate of a Chemical Reaction
... According to kinetic theory (do you remember this?) as the temperature increases the particles in a substance move about more quickly. Reaction at 300C ...
... According to kinetic theory (do you remember this?) as the temperature increases the particles in a substance move about more quickly. Reaction at 300C ...
CHM 122 Chapter 8 -Thermochemistry: Chemical Energy
... Heat: The amount of thermal energy transferred from one object to another as the result of a temperature difference between the two Thermal Energy: The kinetic energy of molecular motion and is measured by finding the temperature of an object We will symbolize heat energy transferred by the letter q ...
... Heat: The amount of thermal energy transferred from one object to another as the result of a temperature difference between the two Thermal Energy: The kinetic energy of molecular motion and is measured by finding the temperature of an object We will symbolize heat energy transferred by the letter q ...
Chemistry and the material world
... N2O4(g) → 2 NO2(g) The connection between the equilibrium constant and the Gibbs free energy: ΔG° = -RT ln K So, to calculate ΔG for a given reaction quotient: ΔG = ΔG° +RT ln Q (note that the expression becomes zero for Q = K) ...
... N2O4(g) → 2 NO2(g) The connection between the equilibrium constant and the Gibbs free energy: ΔG° = -RT ln K So, to calculate ΔG for a given reaction quotient: ΔG = ΔG° +RT ln Q (note that the expression becomes zero for Q = K) ...
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.