Notes
... use the equation to make a table of initial concentrations calculate Q, compare to K and predict direction of reaction represent the change in one concentration as x and use the mol relationships to define the changes in all other species in terms of x sum the initial concentration and the change re ...
... use the equation to make a table of initial concentrations calculate Q, compare to K and predict direction of reaction represent the change in one concentration as x and use the mol relationships to define the changes in all other species in terms of x sum the initial concentration and the change re ...
BASIC CHEMICAL CONCEPTS
... Substances commonly keep their colour when they change form. There are, however, exceptions, especially among changes taking place at high temperatures or pressures (e.g., when mercury boils it gives a colourless gas). In these cases, the question arises, has the substance changed form, or into anot ...
... Substances commonly keep their colour when they change form. There are, however, exceptions, especially among changes taking place at high temperatures or pressures (e.g., when mercury boils it gives a colourless gas). In these cases, the question arises, has the substance changed form, or into anot ...
CHAPTER-7 EQUILIBRIUM Equilibrium state- When
... substance that provides more of an ionic species already present in the dissociation equilibrium. Hydrolysis of Salts: process of interaction between water andcations/anions or both of salts is calledhydrolysis. The cations (e.g., Na+, K+,Ca2+, Ba2+, etc.) of strong bases and anions(e.g., Cl–, B ...
... substance that provides more of an ionic species already present in the dissociation equilibrium. Hydrolysis of Salts: process of interaction between water andcations/anions or both of salts is calledhydrolysis. The cations (e.g., Na+, K+,Ca2+, Ba2+, etc.) of strong bases and anions(e.g., Cl–, B ...
as a PDF
... from 1.68 to 2.13 bar. The 23 H-atom profiles obtained from the 1hexene experiments were measured at temperatures between 1253 and 1398 K and pressures between 1.48 and 2.02 bar. Peukert et al. recommended a 13-step reaction model, which is listed in Table 1. They stated that this mechanism is suffici ...
... from 1.68 to 2.13 bar. The 23 H-atom profiles obtained from the 1hexene experiments were measured at temperatures between 1253 and 1398 K and pressures between 1.48 and 2.02 bar. Peukert et al. recommended a 13-step reaction model, which is listed in Table 1. They stated that this mechanism is suffici ...
Chemical Equilibrium - Request a Spot account
... (endothermic) will become dominant. As the temperature is decreased, the reaction that counteracts that effect (exothermic) will become dominant. Consequently, by observing a chemical system at equilibrium at two different temperatures, the forward reaction can be identified as endothermic or exothe ...
... (endothermic) will become dominant. As the temperature is decreased, the reaction that counteracts that effect (exothermic) will become dominant. Consequently, by observing a chemical system at equilibrium at two different temperatures, the forward reaction can be identified as endothermic or exothe ...
Review Unit 8 Test (Chp 15,17)
... Greater pressure of reactant initially (Q = 0/1.00 = 0) so forward rate is faster due to greater collision frequency of reactant particles. The forward rate slows over time as reactant is consumed and there is a lower collision frequency of reactant particles, but it does not reach zero b/c more rea ...
... Greater pressure of reactant initially (Q = 0/1.00 = 0) so forward rate is faster due to greater collision frequency of reactant particles. The forward rate slows over time as reactant is consumed and there is a lower collision frequency of reactant particles, but it does not reach zero b/c more rea ...
A matter of Equilibrium
... Although rarely include it in the expression for K, instead of using the partial pressure Px of a component we really should use Px/Pref, so that K is then dimensionless. Pref is the standard pressure. This should be 1 bar, but older books (and some new ones) will have used 1 atm. This can make a di ...
... Although rarely include it in the expression for K, instead of using the partial pressure Px of a component we really should use Px/Pref, so that K is then dimensionless. Pref is the standard pressure. This should be 1 bar, but older books (and some new ones) will have used 1 atm. This can make a di ...
Document
... with a high rate. Some reactions take hundreds, maybe even thousands, of years while others can happen in less than one second. If you want to think of a very slow reaction, think about how long it takes plants and ancient fish to become fossils (carbonization). Ultimately: Molecules moving too slow ...
... with a high rate. Some reactions take hundreds, maybe even thousands, of years while others can happen in less than one second. If you want to think of a very slow reaction, think about how long it takes plants and ancient fish to become fossils (carbonization). Ultimately: Molecules moving too slow ...
Acid K a
... NO3- - worthless, NH4+ - weak acid, acidic K+ - worthless, I- - worthless, neutral Li+ - worthless, C2H3O2- - weak base, basic Cl- - worthless, C6H5NH3+ - weak acid, acidic K+ - worthless, F- - weak base, basic ...
... NO3- - worthless, NH4+ - weak acid, acidic K+ - worthless, I- - worthless, neutral Li+ - worthless, C2H3O2- - weak base, basic Cl- - worthless, C6H5NH3+ - weak acid, acidic K+ - worthless, F- - weak base, basic ...
In Class Overview of Chapter
... In this chapter we will learn what determines the extent of a reaction. Thermodynamics is a powerful tool in chemistry, physics and engineering. In chapter 14, we learned about how fast reactions occur, in this chapter we will learn how far a reaction will go. Keep in mind that kinetics and thermody ...
... In this chapter we will learn what determines the extent of a reaction. Thermodynamics is a powerful tool in chemistry, physics and engineering. In chapter 14, we learned about how fast reactions occur, in this chapter we will learn how far a reaction will go. Keep in mind that kinetics and thermody ...
1st Law Of Thermodynamics Part 2
... The differences between Eqn 4 and Eqn 5: 1. We do not write ∆q because q is not a state function and energy supplied as heat cannot be expressed as qf-qi. 2. We must specified the path of integration because q depends on the path selected (example: and adiabatic path has q=0, whereas on the non-adi ...
... The differences between Eqn 4 and Eqn 5: 1. We do not write ∆q because q is not a state function and energy supplied as heat cannot be expressed as qf-qi. 2. We must specified the path of integration because q depends on the path selected (example: and adiabatic path has q=0, whereas on the non-adi ...
2)](http://s1.studyres.com/store/data/015968611_1-56df287e8435abc2be6b0a2948d2417f-300x300.png)
([Cu(NH3)4](MnO4)2)
... starting with an explosion-like reaction at 758. The gas-phase decomposition products are NH3 , O2 , and oxidation products of NH3 , namely N2 , NO, NO2 , and H2O. The presence of N2O could not be detected. Nitrogen oxides and N2 may be formed from direct oxidation of NH3 . The primary oxidation pro ...
... starting with an explosion-like reaction at 758. The gas-phase decomposition products are NH3 , O2 , and oxidation products of NH3 , namely N2 , NO, NO2 , and H2O. The presence of N2O could not be detected. Nitrogen oxides and N2 may be formed from direct oxidation of NH3 . The primary oxidation pro ...
Solution-Solubility-Equilibrium
... There is evidence to suggest that molecules of the solute continue to leave the solid and pass into the solution, while other molecules of solute, previously dissolved, return to the solid state from the solution. To explain the constant macroscopic properties the rate of these two opposing processe ...
... There is evidence to suggest that molecules of the solute continue to leave the solid and pass into the solution, while other molecules of solute, previously dissolved, return to the solid state from the solution. To explain the constant macroscopic properties the rate of these two opposing processe ...
Equilibrium - Tenafly High School
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
Equilibrium - AP Chemistry
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
The Equilibrium Constant
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
... Equilibrium: the extent of a reaction In stoichiometry we talk about theoretical yields, and the many reasons actual yields may be lower. Another critical reason actual yields may be lower is the reversibility of chemical reactions: some reactions may produce only 70% of the product you may calcula ...
File
... (b) On the same diagram indicate the change or changes that result from the addition of the catalyst. Explain the role of the catalyst in changing the rate of the reaction. (c) If the temperature is increased, will the ratio kf/kr increase, remain the same, or decrease? Justify your answer with a on ...
... (b) On the same diagram indicate the change or changes that result from the addition of the catalyst. Explain the role of the catalyst in changing the rate of the reaction. (c) If the temperature is increased, will the ratio kf/kr increase, remain the same, or decrease? Justify your answer with a on ...
Lecture notes
... system then the energy of the system and its surroundings change. Within a chemical system the sum of all kinetic and potential energy, or total energy is called the internal energy, Eint or U. A system contains only internal enemy and not heat and work, which are the means for energy transfer betwe ...
... system then the energy of the system and its surroundings change. Within a chemical system the sum of all kinetic and potential energy, or total energy is called the internal energy, Eint or U. A system contains only internal enemy and not heat and work, which are the means for energy transfer betwe ...
Principles of Chemical Thermodynamics and Kinetics
... A state function is a property of a system that depends upon its current condition only. It will not matter how one arrives at that condition. These functions could include E (energy change), U (internal energy change), H (enthalpy change), S (entropy change), or G (Gibbs free energy change). E ...
... A state function is a property of a system that depends upon its current condition only. It will not matter how one arrives at that condition. These functions could include E (energy change), U (internal energy change), H (enthalpy change), S (entropy change), or G (Gibbs free energy change). E ...
File
... following reversible reactions. a) C3H7OH(l) + CH3COOH(l) CH3COOC3H7(l) + H2O(l) b) 2H2(g) + O2(g) 2H2O(g) c) NH4Cl (s) NH3 (g) + HCl(g) 5. At 25 °C, Kc =0.0146 for the following reaction: PCl5 PCl3 + Cl2 If, at equilibrium, the molar concentrations for PCl5 and PCl3 are 0.500 M and 0.200 ...
... following reversible reactions. a) C3H7OH(l) + CH3COOH(l) CH3COOC3H7(l) + H2O(l) b) 2H2(g) + O2(g) 2H2O(g) c) NH4Cl (s) NH3 (g) + HCl(g) 5. At 25 °C, Kc =0.0146 for the following reaction: PCl5 PCl3 + Cl2 If, at equilibrium, the molar concentrations for PCl5 and PCl3 are 0.500 M and 0.200 ...
kinetics and equilibrium
... • This view of the second law of thermodynamics is very popular, and it has been misused. Some argue that the second law of thermodynamics means that a system can never become more orderly. Not true. It just means that in order to become more orderly (for entropy to decrease), you must transfer ener ...
... • This view of the second law of thermodynamics is very popular, and it has been misused. Some argue that the second law of thermodynamics means that a system can never become more orderly. Not true. It just means that in order to become more orderly (for entropy to decrease), you must transfer ener ...
Chemical Equilibrium - Chemistry with Mrs. Caruso Let the Bonding
... Ex. Suppose there is an equilibrium position described by the concentrations: N2+ 3H2 ⇌ 2NH3 [N2]= .399M; [H2]= 1.197M; [NH3]= .202M What will happen if 1.000 M of N2 is added to the system at constant volume? Will shift to the right. 2. Change in Pressure or Volume: Only for Gases!!!! If _____incre ...
... Ex. Suppose there is an equilibrium position described by the concentrations: N2+ 3H2 ⇌ 2NH3 [N2]= .399M; [H2]= 1.197M; [NH3]= .202M What will happen if 1.000 M of N2 is added to the system at constant volume? Will shift to the right. 2. Change in Pressure or Volume: Only for Gases!!!! If _____incre ...
Please do not remove this page. The periodic table, constants, and
... Consider the balanced equation given for the reaction of iodate ion with iodide ion in acidic solution: IO3– (aq) + 5 I– (aq) + 6 H+ (aq) 3 I2 (aq) + 3 H2O (l) At a particular instant in time, the value of ∆[I–]/∆t = 4.0 x 10–3 M•s–1. What is the value of ∆[I2]/∆t at the same instant in ...
... Consider the balanced equation given for the reaction of iodate ion with iodide ion in acidic solution: IO3– (aq) + 5 I– (aq) + 6 H+ (aq) 3 I2 (aq) + 3 H2O (l) At a particular instant in time, the value of ∆[I–]/∆t = 4.0 x 10–3 M•s–1. What is the value of ∆[I2]/∆t at the same instant in ...
Document
... Catalyst increases the rate of a chemical reaction ◦ Provide a new, lower energy pathway ◦ Forward and reverse reactions pass through the same transition state ◦ Rate for forward and reverse reactions increase by the same factor ◦ Does not affect the composition of the equilibrium mixture ◦ Does not ...
... Catalyst increases the rate of a chemical reaction ◦ Provide a new, lower energy pathway ◦ Forward and reverse reactions pass through the same transition state ◦ Rate for forward and reverse reactions increase by the same factor ◦ Does not affect the composition of the equilibrium mixture ◦ Does not ...
Chemical Equilibrium Equilibrium A state where the reactants and
... Knowing the equilibrium constant allows us to predict several important features of the reaction. 1) the tendency of the reaction to ___________ (but not the _______________) 2) whether a given set of concentrations represent an __________________ condition 3) the equilibrium position that will be ...
... Knowing the equilibrium constant allows us to predict several important features of the reaction. 1) the tendency of the reaction to ___________ (but not the _______________) 2) whether a given set of concentrations represent an __________________ condition 3) the equilibrium position that will be ...