Last 4 Digits of USC ID:____ ____ ____ ____ Dr.
... 4. There are 10 problems on 10 pages. Please count them before you begin. A periodic table and some useful equations can be found on the last page. ...
... 4. There are 10 problems on 10 pages. Please count them before you begin. A periodic table and some useful equations can be found on the last page. ...
Lewis Acids and Bases - Screenshot for timg.co.il
... A 2.00 M AgNO3 aqueous solution is slowly added from a buret to an aqueous solution of 0.0100 M Cl– and 0.0100 M I–. a. Which ion, Cl– or I–, is the first to precipitate from solution? b. When the second ion begins to precipitate, what is the remaining concentration of the first ion? c. Is separatio ...
... A 2.00 M AgNO3 aqueous solution is slowly added from a buret to an aqueous solution of 0.0100 M Cl– and 0.0100 M I–. a. Which ion, Cl– or I–, is the first to precipitate from solution? b. When the second ion begins to precipitate, what is the remaining concentration of the first ion? c. Is separatio ...
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1E5 CHEMISTRY [5 credits]
... Thermodynamics: First law, internal energy, enthalpy; introduction to entropy, 2nd and 3rd Laws; criterion for chemical change; equilibrium constant for a chemical reaction, Gibbs free energy. Physical Chemistry II States of matter: Gibbs phase rule, ideal solutions, colligative properties; Ch ...
... Thermodynamics: First law, internal energy, enthalpy; introduction to entropy, 2nd and 3rd Laws; criterion for chemical change; equilibrium constant for a chemical reaction, Gibbs free energy. Physical Chemistry II States of matter: Gibbs phase rule, ideal solutions, colligative properties; Ch ...
Chem 321 Lecture 11 - Chemical Activities
... Although the calculated pH appears to be only sightly lower than that determined before (4.10), note that the calculated equilibrium [H3O+] is actually 60% higher than that gotten by ignoring ionic interactions. This suggests that the weak acid is ionized to a greater extent than previously expected ...
... Although the calculated pH appears to be only sightly lower than that determined before (4.10), note that the calculated equilibrium [H3O+] is actually 60% higher than that gotten by ignoring ionic interactions. This suggests that the weak acid is ionized to a greater extent than previously expected ...
I PUC Chemistry Mock Paper
... a) Explain Born- Haber cycle for the formation of one mole of NaCl b) Distinguish between closed and isolated system. ...
... a) Explain Born- Haber cycle for the formation of one mole of NaCl b) Distinguish between closed and isolated system. ...
Final Exam - Seattle Central College
... – Let x=change in conc. or partial pressure. 4. Substitute equilibrium conc. or pressures into equilibrium expression for Kp or Kc. 5. Solve for x, using quadratic method if necessary. 6. Substitute value for x into equilibrium conc. or pressures to solve for Kp or Kc. Le Chatelier's Principle – A s ...
... – Let x=change in conc. or partial pressure. 4. Substitute equilibrium conc. or pressures into equilibrium expression for Kp or Kc. 5. Solve for x, using quadratic method if necessary. 6. Substitute value for x into equilibrium conc. or pressures to solve for Kp or Kc. Le Chatelier's Principle – A s ...
Salt Solutions Ionic Bonding
... NaCl is added to water. Like all equilibria, an equilibrium constant is equal to the ratio of the concentrations of products to the concentrations of reactants. The concentration of any solid is defined as 1. The concentration of pure water is a constant, 55.556 M. By multiplying the equilibrium con ...
... NaCl is added to water. Like all equilibria, an equilibrium constant is equal to the ratio of the concentrations of products to the concentrations of reactants. The concentration of any solid is defined as 1. The concentration of pure water is a constant, 55.556 M. By multiplying the equilibrium con ...
CHEMISTRY FINAL EXAM REVIEW SHEET
... Proton: +1 charge, located in nucleus, relative mass = 1 amu Neutron: No charge, located in nucleus, relative mass = 1 amu Electron: -1 charge, located outside of nucleus, relative mass = 1/1840 amu Atomic Number = number of protons in an element. Mass Number = number of protons + neutrons in an ele ...
... Proton: +1 charge, located in nucleus, relative mass = 1 amu Neutron: No charge, located in nucleus, relative mass = 1 amu Electron: -1 charge, located outside of nucleus, relative mass = 1/1840 amu Atomic Number = number of protons in an element. Mass Number = number of protons + neutrons in an ele ...
The Ka values of water and the hydronium ion for comparison with
... would proceed to the right unambiguously showing that acetic acid is a stronger acid than propionic acid in aqueous solution. In this case, the acids are on "equal terms", and a comparison of the K.s' for these acids yields a valid result. However, when one compares a compound's acid strength with t ...
... would proceed to the right unambiguously showing that acetic acid is a stronger acid than propionic acid in aqueous solution. In this case, the acids are on "equal terms", and a comparison of the K.s' for these acids yields a valid result. However, when one compares a compound's acid strength with t ...
Packet 2- Chemistry of Life
... 2. Enzymes are proteins that catalyze chemical reactions 3. Receptors are proteins that bind to signal molecules (like hormones) and then initiate some sort of cellular response. 4. Transporters are proteins that help substances move in and out of a cell. ...
... 2. Enzymes are proteins that catalyze chemical reactions 3. Receptors are proteins that bind to signal molecules (like hormones) and then initiate some sort of cellular response. 4. Transporters are proteins that help substances move in and out of a cell. ...
Condensed Matter 2
... is the value of Qc when the reaction is at equilibrium. The ratio Kc/Qc serves as an index how the composition of the reaction system compares to that of the equilibrium state. Thus, it indicates the direction in which any net reaction must proceed. ...
... is the value of Qc when the reaction is at equilibrium. The ratio Kc/Qc serves as an index how the composition of the reaction system compares to that of the equilibrium state. Thus, it indicates the direction in which any net reaction must proceed. ...
Transition Metals - Ligand Stability and Chelation
... When considering a reaction, remember that the Gibbs’ free energy (ΔG) must always be ≤0 for a reaction to occur spontaneously. This means that the TΔS function must be greater than the ΔH function. This is why reactions generally occur more spontaneously at higher temperatures. When adding a multid ...
... When considering a reaction, remember that the Gibbs’ free energy (ΔG) must always be ≤0 for a reaction to occur spontaneously. This means that the TΔS function must be greater than the ΔH function. This is why reactions generally occur more spontaneously at higher temperatures. When adding a multid ...
Q1) Discuss the following briefly: (a) The effect of hydrogen bond on
... partially miscible. A final type exhibits no critical solution temperature; the pair ethyl ether and water, for example, has neither an upper nor a lower critical temperature and shows partial miscibility over the entire temperature range at which the mixture exists. ...
... partially miscible. A final type exhibits no critical solution temperature; the pair ethyl ether and water, for example, has neither an upper nor a lower critical temperature and shows partial miscibility over the entire temperature range at which the mixture exists. ...
Equilibrium chemistry
Equilibrium chemistry is a concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero. This principle, applied to mixtures at equilibrium provides a definition of an equilibrium constant. Applications include acid-base, host-guest, metal-complex, solubility, partition, chromatography and redox equilibria.