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Chapter 11.1: Describing Chemical Reactions
... catalyst is a substance that can be added to speed up the reaction but is not used up in a reaction. It is neither a product or a reactant. ...
... catalyst is a substance that can be added to speed up the reaction but is not used up in a reaction. It is neither a product or a reactant. ...
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 ...
AP Chemistry Test Review
... 39) more O’s in the oxy-acid means easier to lose the H+, therefore it is a stronger acid 40) salts made of metals in the d-block that have multiple charges are usually colorful solutions 41) common ion effect…less likely to ionize or dissolve 42) NaHCO3 is baking soda and releases CO2(g) in most re ...
... 39) more O’s in the oxy-acid means easier to lose the H+, therefore it is a stronger acid 40) salts made of metals in the d-block that have multiple charges are usually colorful solutions 41) common ion effect…less likely to ionize or dissolve 42) NaHCO3 is baking soda and releases CO2(g) in most re ...
Collision Theory
... • Before atoms/molecules/ions can react, they must first collide • An effective collision between two species puts enough energy to break key bonds • The activation energy (Ea) is the minimum energy that must be supplied by collisions to trigger a reaction • A certain fraction of all molecules in a ...
... • Before atoms/molecules/ions can react, they must first collide • An effective collision between two species puts enough energy to break key bonds • The activation energy (Ea) is the minimum energy that must be supplied by collisions to trigger a reaction • A certain fraction of all molecules in a ...
Chapter 4
... - the concentration of water in dilute solutions is very large compared with the concentration of hydrogen and hydroxide ions, so the concentration of water can be re-written as the ion product constant for water: K[H2O]2 = Kw = [H3O+] [OH-] Because OH- and H3O+ are formed only from the dissociation ...
... - the concentration of water in dilute solutions is very large compared with the concentration of hydrogen and hydroxide ions, so the concentration of water can be re-written as the ion product constant for water: K[H2O]2 = Kw = [H3O+] [OH-] Because OH- and H3O+ are formed only from the dissociation ...
Equilibrium Review True/False Indicate whether the statement is
... 1. (1 point) What three characteristics are common to all reactions that have reached equilibrium. 2. (1 point) Write the equilibrium constant expression for the following reaction: A (s) + 3B (g) + 5C (g) 2D (s) + 1E (1) 3. (1 point) Explain why equilibrium will be unaffected if the pressure of t ...
... 1. (1 point) What three characteristics are common to all reactions that have reached equilibrium. 2. (1 point) Write the equilibrium constant expression for the following reaction: A (s) + 3B (g) + 5C (g) 2D (s) + 1E (1) 3. (1 point) Explain why equilibrium will be unaffected if the pressure of t ...
File - Chem with Appleby
... SECTION 4: Homogenous vs. Heterogeneous-15 • Homogeneous equilibria: ________________________________ ________________________________ ________________________________ ________________________________ • Heterogeneous equilibria: ________________________________ ________________________________ _____ ...
... SECTION 4: Homogenous vs. Heterogeneous-15 • Homogeneous equilibria: ________________________________ ________________________________ ________________________________ ________________________________ • Heterogeneous equilibria: ________________________________ ________________________________ _____ ...
Chemical Equilibrium
... and vibration from appropriate input data • Define chemical equilibrium in terms of occupation numbers and microstates • Write down and explain the general definition of the equilibrium constant for an isomerization reaction ...
... and vibration from appropriate input data • Define chemical equilibrium in terms of occupation numbers and microstates • Write down and explain the general definition of the equilibrium constant for an isomerization reaction ...
NAME REVIEW 1: JUST THE BASICS ___1) In which material are
... 20) 1) HI it is produced endothermically and that means more energy is absorbed by the breaking of bonds than is released as the new H-I polar covalent bond(s) is (are) produced. Thus HI is less stable than the reactants. 21) 3 an increase in temp favors the endo. rxn which in this case is the forwa ...
... 20) 1) HI it is produced endothermically and that means more energy is absorbed by the breaking of bonds than is released as the new H-I polar covalent bond(s) is (are) produced. Thus HI is less stable than the reactants. 21) 3 an increase in temp favors the endo. rxn which in this case is the forwa ...
Chapter 16 Handout
... reactions have not ceased. They occur simultaneously at the same rate. During dynamic equilibrium: –The ____________________. and concentrations of chemical substances remain constant. –The total gas ____________________. is constant (if gases are involved) –The ____________________. us constant –Th ...
... reactions have not ceased. They occur simultaneously at the same rate. During dynamic equilibrium: –The ____________________. and concentrations of chemical substances remain constant. –The total gas ____________________. is constant (if gases are involved) –The ____________________. us constant –Th ...
Chemical Equations and Reactions notes File
... Whole numbers in front of formula Distributes to numbers of atoms in formula specifies the number of moles in the reaction used to balance the equation ...
... Whole numbers in front of formula Distributes to numbers of atoms in formula specifies the number of moles in the reaction used to balance the equation ...
Chemical Equilibrium is reached when
... However, in 1 L of water we have 55.5 M of water which is very large compared with the concentrations of other species in solution, and we assume that it doesn’t change during the course of a reaction. Kc = [CH3COO-][H3O+]/[CH3COOH] Kc = Kc`[H2O] Note that it is general practice not to include units ...
... However, in 1 L of water we have 55.5 M of water which is very large compared with the concentrations of other species in solution, and we assume that it doesn’t change during the course of a reaction. Kc = [CH3COO-][H3O+]/[CH3COOH] Kc = Kc`[H2O] Note that it is general practice not to include units ...
Every reaction is reversible: A chemical reaction is in equilibrium
... 0.1 mol C2H4 was allowed to react with 0.04 mol CH3COOH at 100C. The total volume was made up to 1 litre with an inert solvent so that all reactants and products will be in the liquid phase. This is described as 'homogeneous equilibrium' - all species are in the same phase. In heterogeneous equilibr ...
... 0.1 mol C2H4 was allowed to react with 0.04 mol CH3COOH at 100C. The total volume was made up to 1 litre with an inert solvent so that all reactants and products will be in the liquid phase. This is described as 'homogeneous equilibrium' - all species are in the same phase. In heterogeneous equilibr ...
Complex Ions and Free Energy
... • Recall that we calculated standard free energies (ΔGo), which were when all concentrations were 1 M and temperature was 298 K. • Most reactions occur at non-standard condition and we can calculate ΔG at this point with: ...
... • Recall that we calculated standard free energies (ΔGo), which were when all concentrations were 1 M and temperature was 298 K. • Most reactions occur at non-standard condition and we can calculate ΔG at this point with: ...
South Pasadena · AP Chemistry
... Chlorine molecules will dissociate at high temperatures into chlorine atoms. At 3000C, for example, Kc for the equilibrium shown is 0.55. If the partial pressure of chlorine molecules is 1.5 atm, calculate the partial pressure of the chlorine atoms: Cl2(g) 2 Cl(g) ...
... Chlorine molecules will dissociate at high temperatures into chlorine atoms. At 3000C, for example, Kc for the equilibrium shown is 0.55. If the partial pressure of chlorine molecules is 1.5 atm, calculate the partial pressure of the chlorine atoms: Cl2(g) 2 Cl(g) ...
Unit 4 Chemical Kinetics and Chemical Equilibrium
... Effects of Changing Pressure and Volume: If Volume decreases, partial pressures of the reactants and products increase: system shifts to reduce pressure ...
... Effects of Changing Pressure and Volume: If Volume decreases, partial pressures of the reactants and products increase: system shifts to reduce pressure ...
Word - chemmybear.com
... Chlorine molecules will dissociate at high temperatures into chlorine atoms. At 3000C, for example, Kc for the equilibrium shown is 0.55. If the partial pressure of chlorine molecules is 1.5 atm, calculate the partial pressure of the chlorine atoms: Cl2(g) 2 Cl(g) ...
... Chlorine molecules will dissociate at high temperatures into chlorine atoms. At 3000C, for example, Kc for the equilibrium shown is 0.55. If the partial pressure of chlorine molecules is 1.5 atm, calculate the partial pressure of the chlorine atoms: Cl2(g) 2 Cl(g) ...
