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The document discusses solubility and solubility products, oxidation-reduction reactions, and voltaic cells. It defines key concepts like reducing agents, oxidizing agents, and half-reactions. It also discusses standard reduction potentials, how to determine if a reaction involves oxidation-reduction, and how to balance half-reactions to indicate oxidation or reduction. Sample problems are provided to calculate equilibrium constants from solubility products and oxidation states in reactions.
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Exam #2 Re-work
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O
Name: _______________________________ (Ex2 rework)
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O
1. LiAlH4
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Name: _______________________________ (Ex2 rework)
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O
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Name: _______________________________ (Ex2 rework)
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Name: _______________________________ (Ex2 rework)
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Chemistry review 4 th period exam 2nd semesterGaby De La Garza
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This document contains a chemistry review for a second semester exam covering topics like organic vs inorganic compounds, properties of organic compounds, carbon bonding, hydrocarbons, functional groups, isomers, acids and bases, pH, and acid rain. It includes multiple choice and short answer questions testing the students understanding of these concepts.4784 et et
4784 et etrammaheswari
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The document discusses various types of organic reactions including substitution, addition, elimination, rearrangement, and oxidation/reduction reactions. It provides examples and mechanisms for each type. Substitution reactions involve replacing one atom or group with another. Addition reactions increase unsaturation by adding atoms or groups across double/triple bonds. Elimination reactions remove two atoms/groups from adjacent carbons to form a multiple bond. Rearrangement reactions involve migration of an atom/group within a molecule. Oxidation/reduction reactions involve gain/loss of electrons.Practice Test 3
Practice Test 3jessieo387_1412
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1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.Adsorption
AdsorptionJefri Ferliande
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This document discusses adsorption, which refers to the accumulation of solutes at solid-solution interfaces in soils. There are two main types of adsorption - physical and chemical. Adsorption is determined through batch or column experiments by measuring the removal of solutes from solution onto an adsorbent. The relationship between the solute adsorbed and its equilibrium concentration is described by adsorption isotherms, with common models including linear, Freundlich, Langmuir, and BET isotherms. Adsorption of ions onto soil surfaces can occur through mechanisms such as electrostatic exchange or covalent bonding, and depends on properties of both the ion and soil surface.ENV 3001 Final Exam_Summer 2015.pdfENV 3001 Name_.docx
ENV 3001 Final Exam_Summer 2015.pdfENV 3001 Name_.docxYASHU40
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ENV 3001 Final Exam_Summer 2015.pdf
ENV 3001 Name:___________________
Final Exam Date: June 18, 2015
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Answer all questions in the space provided and transfer your answers to the answer sheet.
1-2. The dilution factor P of an unseeded mixture of liquid wastewater is 0.03. The initial DO of the
mixture is 10.0 mg/L. After 5 days, DO has dropped to 1.0 mg/L.
Assuming: Reaction rate constant k = 0.22 day
-1
.
1. The 5-day BOD of the waste is most nearly:
a. 600 mg/L
b. 500 mg/L
c. 400 mg/L
d. 300 mg/L
e. 200 mg/L
f. other, write your answer _________________
2. The ultimate BOD of the liquid waste would be most nearly:
a. 550 mg/L
b. 450 mg/L
c. 350 mg/L
d. 240 mg/L
e. 150 mg/L
f. other, write your answer _________________
3-4. A water sample has the following analysis:
Concentration (mg/L) Atomic/ionic weight
Ca
+2
80 40
Mg
+2
30 24.4
Na
+
72 23
K
+
6 39
Cl
-
100 35.5
SO4
-2
201 96
HCO3
-
162 61
3. Total hardness of the water is most nearly (as mg/L as CaCO3):
a. 479 mg/L
b. 344 mg/L
c. 323 mg/L
d. 200 mg/L
e. 135 mg/L
f. other, write your answer _________________
4. Total carbonate harness is most nearly (as mg/L as CaCO3):
a. 479 mg/L
b. 441 mg/L
c. 323 mg/L
d. 266 mg/L
e. 133 mg/L
f. other, write your answer _________________
5. NO2 concentration in air is measures as 0.25 ppm at 25
o
C and 1 atm pressure. The concentration
of NO2 in µg/m
3
is most nearly:
Atomic weights: N: 14 O: 16
a. 770
b. 640
c. 520
d. 470
e. 320
f. other, write your answer _________________
6-8. A rural community of 20,000 persons generates solid waste at an average rate of 7 lbs
per person per day. A ...Chemistry - Chp 18 - Reaction Rates and Equilibrium - Notes
Chemistry - Chp 18 - Reaction Rates and Equilibrium - NotesMr. Walajtys
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The document discusses chemical reaction rates and equilibrium. [1] It describes how reaction rates are expressed based on the amount of reactant changing over time and discusses collision theory, in which reactions only occur when collisions reach the minimum energy of activation. [2] It identifies four factors that influence reaction rates: temperature, concentration, surface area, and presence of a catalyst. [3] The document also discusses chemical equilibrium, how systems at equilibrium can be disturbed by changes in concentration, temperature, or pressure based on Le Chatelier's principle, and how the equilibrium constant Keq indicates whether reactants or products are favored.Si #12
Si #12Lamar1411_SI
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This document defines key chemistry terms and concepts related to aqueous solutions, electrolytes, acids and bases, precipitation reactions, and solubility. It asks the student to identify strong acids and bases, ions present when various substances dissolve in water, solubility of compounds, precipitation reactions, and classification of solutions as nonelectrolytes, weak electrolytes, or strong electrolytes. The document provides a review of general chemistry topics through multiple choice and short answer questions.Understanding the Chemistry Reference Tables Lab w/ Key
Understanding the Chemistry Reference Tables Lab w/ KeyRyan Frank
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Lab assessment to help students understand how to use the Chemistry Reference Tables. It can be used for all versions, but the 2011 is the version that the key was made for. Chemistry - Chp 20 - Oxidation Reduction - Notes
Chemistry - Chp 20 - Oxidation Reduction - NotesMr. Walajtys
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Oxidation and reduction reactions, also called redox reactions, involve the transfer of electrons between reactants. In redox reactions, one reactant gets oxidized by losing electrons while another reactant gets reduced by gaining electrons. The reactant that loses electrons is the oxidizing agent, while the reactant that gains electrons is the reducing agent. Redox reactions can be identified by changes in oxidation numbers, which are assigned to track electron gains and losses. Balancing redox equations requires splitting the overall reaction into separate half-reactions for oxidation and reduction, then combining the half-reactions by adding electrons to balance charges.
Class 12 Cbse Chemistry 2010 Sample Paper Model 2 
Class 12 Cbse Chemistry 2010 Sample Paper Model 2 Sunaina Rawat
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cbse class 12 chemistry 2010 sample paper model 2 - http://cbse.edurite.com/cbse-sample-papers-2010.htmlTypes of chemical reactions document
Types of chemical reactions documentJudy Fitzpatrick
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1. This document discusses different types of chemical reactions including synthesis, decomposition, single replacement, double replacement, and combustion reactions.
2. It provides examples of equations for each type of reaction and asks questions to test understanding of classifying reactions and identifying the products.
3. Key points covered include the definitions of synthesis as two reactants forming one product, decomposition as one reactant breaking into two or more products, and double replacement as two compounds exchanging ions to form two new compounds.Chemical Reaction Worksheet for STEM Students.doc
Chemical Reaction Worksheet for STEM Students.docclaresa1
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An adaptation. Credit goes to the original author. Ap chemistry notes chapter 1
Ap chemistry notes chapter 1Sherri Mazzone
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Chemistry is the study of matter and its composition and changes. Matter is composed of elements and compounds. The main areas of study in chemistry include organic chemistry, inorganic chemistry, analytical chemistry, physical chemistry, biochemistry. [Chemistry notes provide an overview of key areas of chemistry including matter, elements, compounds, mixtures, states of matter, and areas of study in chemistry such as organic, inorganic, analytical, physical, and biochemistry.]Ch8 balance equations vocab
Ch8 balance equations vocabJeff Kalember
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This document provides vocabulary terms for different types of chemical reactions:
1) Precipitate refers to the chunky stuff that falls to the bottom of a test tube in a double replacement reaction.
2) Decomposition reactions involve ABC yielding A + B + C, while synthesis reactions involve AB + CD yielding AD + CB.
3) Double replacement reactions involve AB + C yielding AC + B, while single replacement reactions involve AB + C yielding AC + B and both B and C must be nonmetals.Attacking the TEKS: Chemical Reactions
Attacking the TEKS: Chemical ReactionsPaul Schumann
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Attacking the TEKS: Focus on Chemical Reactions presented by Claudia Wallace, ACT2 2010
This session will expose you to the new iEKS and College Readiness Standards. Ideas for sequencing and planning the unit will be shared along with tips for appropriate demos, labs, and assessments. The intended audience is for teachers with 3 or less years of experience or anyone who wants to delve deeper into the new standards. More from jessieo387_1412 (12)
#27
#27jessieo387_1412
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This document contains questions about oxidation-reduction reactions and voltaic cells. It asks the student to identify oxidizing and reducing agents, write half reactions, identify anodes and cathodes, and determine the direction of electron and ion flow. It also contains questions about standard cell potentials, units of electrical potential, and a half reaction for a hydrogen electrode.#25 Key
#25 Keyjessieo387_1412
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1. The common ion effect decreases the ionization of a weak electrolyte when a strong electrolyte with a common ion is added to the solution.
2. Buffer capacity refers to how much acid or base can be neutralized before the pH begins to change significantly.
3. A buffer solution contains a weak acid or base and its salt. It has the ability to resist changes in pH.
4. The pH range of a buffer depends on the acid's Ka value and the relative concentrations of the acid and base in the buffer solution. It is the range over which the buffer acts effectively.#24 Key
#24 Keyjessieo387_1412
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This document provides examples of calculating the pH of various strong acid solutions, including nitric acid, perchloric acid, hydrochloric acid, a mixture of hydrochloric acid and hydroiodic acid, and a solution of bromoacetic acid that is partially ionized. It also asks questions about weak acids, Lewis acids, and which compounds form more acidic solutions based on cation properties.#20 Key
#20 Keyjessieo387_1412
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The document provides information about acid-base chemistry including:
1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions.
2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values.
3) Relating pH and pOH through the equation pH + pOH = 14.
4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.#19 Key
#19 Keyjessieo387_1412
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This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.#18 Key
#18 Keyjessieo387_1412
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The document contains 6 chemistry problems involving gas phase chemical equilibria calculations:
1) Calculating the equilibrium partial pressure of N2O4 and the equilibrium constant Kp for the reaction N2O4 ⇌ 2NO2.
2) Calculating the equilibrium concentrations of H2, Br2, and HBr and the equilibrium constant Kc for the reaction H2 + Br2 ⇌ 2HBr.
3) Calculating the equilibrium constant Kc for the reaction SO2 + Cl2 ⇌ SO2Cl2 given the value of Kp.
4) Calculating the value of Kp for the reverse reaction of 2NO2 ⇌#17 Key
#17 Keyjessieo387_1412
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1. The document contains 7 chemistry problems involving calculation of equilibrium constants (Keq and Kc) for various chemical reactions.
2. Problem 3 calculates Keq as 1.84x10-2 for the decomposition of HI gas into H2 and I2 gases at 425C, given the partial pressures of reactants and products at equilibrium.
3. Problem 7 involves a multiple step chemical equilibrium problem, calculating the initial and equilibrium partial pressures and concentrations of gases in a reaction between CO2, H2 and H2O, and determining the equilibrium constant Kp.SI #13 Key
SI #13 Keyjessieo387_1412
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This document contains information about several chemistry concepts and example calculations:
1) It provides calculations to determine the amount of N2O5 remaining and reaction time for its decomposition reaction at 70°C.
2) It discusses how reaction rates change with changes in reactant concentrations for a reaction following a rate law.
3) It gives the rate law and calculates rates for the decomposition of N2O5 in carbon tetrachloride.
4) It provides the rate law and calculates rates for a reaction that is 1st order in H2 and 2nd order in NO.
5) It states that the law of mass action expresses the relationship between reactant and product concentrations at equilibrium.Si #12 Key
Si #12 Keyjessieo387_1412
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1. Chemical kinetics is the study of time vs. the rate of chemical change. The three factors that affect chemical reactions are concentration, temperature, and catalysts.
2. Instantaneous rate is the slope of a line drawn tangent to the concentration-time curve at a specific time. Beer's Law states that absorption of electromagnetic radiation by a substance is directly proportional to its concentration.
3. A first-order reaction has a rate proportional to the concentration of a single reactant raised to the first power. The rate is equal to k[A] and a plot of ln[A] versus time gives a straight line with a slope of -k.#11 Key
#11 Keyjessieo387_1412
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The document contains a chemistry problem set with 10 questions:
1) It asks to calculate the molarity of three aqueous solutions.
2) It asks to calculate the percentage by mass of nitric acid in a 16 M commercial solution.
3) It asks to calculate the osmotic pressure of a solution formed by dissolving aspirin in water.
4) It asks to order solutions by increasing boiling point.
5) It defines hydrophobic and hydrophilic colloids and provides examples.
6) It asks to identify colloids as hydrophobic or hydrophilic.#9 Key
#9 Keyjessieo387_1412
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London dispersion forces are the attractive force between two molecules with hydrogen bonded to the oxygen atom. CH4 has dispersion forces as its only intermolecular force. Adsorption is the process of a substance sticking to the surface of another. Surface tension is the energy required to expand the surface area of a liquid by a unit amount of area. The vapor pressure of any substance at its normal boiling point is 1 atm. The concentration of nitrate ion in a solution containing 0.900 M aluminum nitrate is 2.70 M. Sublimination is the direct conversion of a solid to a gas.#8 Key
#8 Keyjessieo387_1412
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1. Ionic bonding involves the complete transfer of an electron from one element to another.
2. Covalent bonds have equally shared pairs of electrons between atoms.
3. Polar covalent bonds are defined as occurring when one atom exerts a greater attraction for the bonding electrons.#26
- 1. GENERAL CHEMISTRY-II (1412) S.I. # 26 1. The Solubility of an y compound in ____________can be converted to ____________. The ____________can be used to determine the____________of ions in a solution. The ____________ of ions can be used to calculate ______. The steps can be __________ and solubility calculated from ___Pg 741 2. Fill in the boxes below: (g/L) (mol/L) ions Ksp 3. Ksp for AgI is 8.3x10-17 (appendix D) and Kf for Ag(CN)2- is 1x1021 (pg750 table 17.1) calculate the equilibrium constant for the reaction AgI(s) + 2CN-(aq) ïƒŸïƒ Ag(CN)2-(aq) + I-(aq) 4. Define reducing agent and oxidizing agent and give their functions. 5. What is a half-reaction? 6. Define anode and cathode in terms of a voltaic cell. 7. What is the function of a salt bridge?
- 2. 8. What is emf? 9. The emf of a cell is called ______________. And when it is under standard conditions it is called _______________. For a half-reaction, _____ is a measure of the tendency of the reduction to occur. The value of _____ is _______ for a voltaic cell and can be found by the equation: ___________________________________. ______________ has the most positive value for _____ and is the strongest oxidizing agent. 10. Indicate whether the following balanced equations involve oxidation-reduction. If they do, identify the elements that undergo changes in oxidation number. A. PBr3(l) + 3 H2O (l) ïƒ H3PO3(aq) + 3 HBr (aq) B.NaI (aq) + 3 HOCl(aq) ïƒ NaIO3 (aq) + 3 HCl (aq) C. 3 SO2(g) + 2 HNO3 + H2O(l) ïƒ 3 H2SO4(aq) + 2 NO(g) D. 2 H2SO4(aq) + 2 NaBr(s) ïƒ Br2(l) + SO2(g) + Na2SO4(aq) 2 H2O (l) 11. complete and balance the half reactions and indicate whether the half is reduction or oxidation. A. Mo3+ ïƒ Mo(s) B. H2SO3(aq) ïƒ SO42-(aq) C. NO3-(aq) ïƒ NO(g) D. Mn2+(aq) ïƒ MnO2(s) E. Cr(OH)3(s) ïƒ CrO42- (aq)