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W7.ans
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LP_calc
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Chemistry 114 Spring 2010 Lab Practical Name: _ 1. For each of the following give 1) the most appropriate Lewis structure, 2) all resonance structures, and 3) formal changes for all atoms having any. a) nitric acid, HNO3 b) hydrogen phosphate ion, HPO2 4

11.5_C_GibbsHelmholtz Equation Calculations
School: Ill. Chicago
For the reaction CaCO3(s) CaO(s) + CO2(g) Go = 127.6 kJ and Ho = 178.3 kJ at 316 K and 1 atm. This reaction is (reactant,product) favored under standard conditions at 316 K. The entropy change for the reaction of 2.38 moles of CaCO3(s) at this temperature

Heat Capacity Definitions1
School: Ill. Chicago
Heat Capacity Definitions The Specific Heat, Csp, of a substance is the energy required to raise the temperature of one gram of the substance, one degree. It is usually reported in units of (Joules/gram oC). The term "specific" means "per gram". The Molar

Functions And Graphs
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Functions and Graphs. (1) Generating points from a function. A function that relates one variable to another can be used to generate points that belong to that function. For example, for the function y = 20  x2 for any value of x, a value of y can be cal

Exponent Algebra Rules
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Exponent Algebra Rules xn xm . = n x / xm . = (xn)m . = 1/xn . = x0 . = Summary xn+m xnm xnm xn 1 Multiply by same variable  Add exponents Divide by same variable  Subtract exponents Raise variable to a power  Multiply exponents Reciprocal of variabl

Energy Unit Conversions
School: Ill. Chicago
Energy Unit Conversions Question: Melting lead requires 5.91 cal/g. How many joules are required to melt 1.5 lb of lead? (1 lb= 454g; 1 cal= 4.18 J) Answer: 16935.44 Heat Equilibrium Question: A 33.7 g sample of copper at 99.8 C is dropped into a beaker c

Direct And Inverse Proportions
School: Ill. Chicago
Direct and Inverse Proportions Two functional forms that are important in chemistry are direct and inverse proportions. Direct proportions. A direct proportion has the form y = ax, where a is a constant. A direct proportion is so called because what is do

Calorimetry_Q1
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Calorimetry Hw3
School: Ill. Chicago
o A chunk of zinc weighing 19.5 grams and originally at 97.85 C is dropped into an insulated cup o containing 80.1 grams of water at 20.59 C. Assuming that all of the heat is transferred to the water, the final temperature of the water is o C. Feedback: H

Calorimetry Hw2
School: Ill. Chicago
An electric range burner weighing 643 grams is turned off after reaching a temperature of 498.0oC, and is allowed to cool down to 22.6oC. Calculate the specific heat of the burner if all the heat evolved from the burner is used to heat 590 grams of water

Calorimetry Hw1
School: Ill. Chicago
A 0.242 g sample of napthalene (C10H8) is burned in a bomb calorimeter containing 1025 g of water. How much will the temperature rise ? o The heat capacity of the calorimeter is 802 J/ C. 3 The heat of combustion of naphthalene is 5.15 x 10 kJ/mol o The

Assignment List
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Heat Capacity Definitions2
School: Ill. Chicago
Heat Capacity Definitions The Specific Heat, Csp, of a substance is the energy required to raise the temperature of one gram of the substance, one degree. It is usually reported in units of (Joules/gram oC). The term "specific" means "per gram". The Molar

Heat Capacity Definitions3
School: Ill. Chicago
Heat Capacity Definitions The Specific Heat, Csp, of a substance is the energy required to raise the temperature of one gram of the substance, one degree. It is usually reported in units of (Joules/gram oC). The term "specific" means "per gram". The Molar

Heat Capacity Definitionschapter 10.1
School: Ill. Chicago
Heat Capacity Definitions The Specific Heat, Csp, of a substance is the energy required to raise the temperature of one gram of the substance, one degree. It is usually reported in units of (Joules/gram oC). The term "specific" means "per gram". The Molar

11.5_C_3Qualitative Delta G, H, S
School: Ill. Chicago
Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following exothermic reaction. 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g) 1) > 0 2) < 0 3) = 0 4) > 0 low T, < 0 high T 5) < 0 low T, > 0 hig

11.5_C_2delta Go Rxn From Formation Data
School: Ill. Chicago
Consider the reaction 2NH3(g) + 3N2O(g) 4N2(g) + 3H2O(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.54 moles of NH3(g) react at standard conditions. o . G rxn = kJ Feedback: Calculate Gorxn from standard free energi

11.4
School: Ill. Chicago
o For benzene, C6H6, the heat of fusion at its normal melting point of 6 C is 10.0 kJ/mol. o 1 The entropy change when 2.13 moles of solid C6H6 melts at 6 C, 1 atm is JK . Feedback: The melting of benzene at its normal melting point is an equilibrium pro

11.3_Entropy And The Second Law
School: Ill. Chicago
Consider the reaction 4HCl(g) + O2(g) 2H2O(g) + 2Cl2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.80 moles of HCl(g) react at standard conditions. . Ssurroundings = J/K Feedback: The entropy of the

11.3_B_Favored From Delta So Universe Calculation
School: Ill. Chicago
Consider the reaction 2NH3(g) + 3N2O(g) 4N2(g) + 3H2O(g) for which o H = 879.5 kJ and o S = 288.1 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.816 moles of NH3(g) react under standard conditions at 298.15 K. Suniverse = J/K (2

11.2_a_balance Half Rxns
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Balancing OxidationReduction Reactions 1. Assign oxidation numbers. 2. Separate into oxidation and reduction half reactions. 3. Balance each half reaction using the following steps: a. Balance all elements except oxygen or hydrogen. b. Balance oxygen by

11.2_ Entropy Change For A Reaction
School: Ill. Chicago
Consider the reaction 2C2H6(g) + 7O2(g) 4CO2(g) + 6H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.59 moles of C2H6(g) react at standard conditions. . Ssystem = J/K Feedback: First calculate S o rxn= So

11.1_Qualitative Entropy
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Arrange the substances on the left in order of increasing entropy. Assume 1 mole of each at standard conditions. 1) lowest entropy SO2(g) 2) 3) S(s) 4) highest entropy SO3(g) O2(g) Feedback: For similar substances in the same state, entropies of more comp

The Slope
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The slopeintercept equation for a straight line. The following points (x,y) x 0 1 2 3 4 y 2 8 14 20 26 generate the following straight line when y is plotted (yaxis) against x (xaxis): A straight line can be represented in the form y = mx + b where b =

OWLalgebra
School: Ill. Chicago
Exponent Algebra Rules xn xm . = n x / xm . = (xn)m . = 1/xn . = x0 . = Summary xn+m xnm xnm xn 1 Multiply by same variable  Add exponents Divide by same variable  Subtract exponents Raise variable to a power  Multiply exponents Reciprocal of variabl

Assignment 1_complete
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12.4_#3
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10.8First Law Of Thermodynamics
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First Law of Thermodynamics When a system exchanges energy with its surroundings in the form of work or heat, the first law may be written: E = q + w where E = change in the internal energy of the system q = energy exchanged between the system and the sur

GRAPH 1
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EMISSION SPECTRA!
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Theemissionspectraofsomeelements INTRODUCTION: thepurposeofthislabistoobservethespectraofdifferentemissionsourcesusinga gratingspectrometerandusespectrometertoidentifytheunknown,Therewillbeasetofunknownsforeach labsection.Wewillalsocalculatetheenergyleve

6)
School: Ill. Chicago
time 5 10 15 20 25 30 35 40 45 50 [CrO3Cl] 2.04E03 2.14E03 2.02E03 1.86E03 1.78E03 1.53E03 1.55E03 1.51E03 1.44E03 1.34E03 [CrO3Cl]^2 4.16E06 4.58E06 4.08E06 3.46E06 3.17E06 2.34E06 2.40E06 2.28E06 2.07E06 1.80E06 5.00E06 f(x) = 1.0

2) Calorimetry And Hess's Law
School: Ill. Chicago
Title: Calorimetry and Hesss Law Course: Chemistry 118 Date: January 22, 2008 INTRODUCTION In this lab, we were to use concepts of calorimetry and Hesss law to determine H. H, change in enthalpy of the reaction, is the change in the heat content of a chem

5) Electrochemical Measurement And Batteries (1)
School: Ill. Chicago
INTRODUCTION In this experiment, we constructed an activity series of metals, such as silver, copper, iron, zinc and determined which metals to use in constructing battery with highest voltage. Even though metals have a strong tendency to give up electron

6) The Rate Of The Oxidation Of Ethanol By Chromium(VI) (1)
School: Ill. Chicago
INTRODUCTION In this experiment, we were to determine the rate of the oxidation of ethanol by Cr(VI) and the order of the reaction. The basic concept of this lab, chemical kinetics is the study of the rates and mechanisms of chemical reactions. The rate o

Theoretical Wavelengths
School: Ill. Chicago
1 2 3 453 579 706 604 704 650 WavelengthsVs.#ofCHChgroupsinthemiddleofthechain 800 f(x) = 126.5x + 326.3333333333 R = 0.9999947924 f(x) = 23x + 606.6666666667 R = 0.2111495476 700 Column B Column C 500 Linear Regression for Column B Linear Regression for

W5.ans
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W4.ans
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W3.ans
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GRAPH 2
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Graph 4
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Graph 3
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10.7_Using Average Bond Enthalpies
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Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: I2(g) + Br2(g) 2IBr(g) kJ Feedback: The enthalpy of a gas phase reaction may be estimated by taking into account the number of bonds broken (Ein > 0) ve

10.7_Bond Enthalpy From Enthalpy Rxn
School: Ill. Chicago
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the NH bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol Feedback: Given the enthalpy of a gas phase reaction, the NH bond energy may be estimated by taking int

10.6Enthalpy And Hess's Law
School: Ill. Chicago
Given the standard enthalpy changes for the following two reactions: o (1) N2(g) + 2 O2(g) 2 NO2(g). H = 66.4 kJ (2) 2 N2O(g) 2 N2(g) + O2(g) . H = 164.2 kJ o what is the standard enthalpy change for the reaction: (3) 2 N2O(g) + 3 O2(g) 4 NO2(g) . o H =?

10.6_Enthalpy Formation From Enthalpy Rxn
School: Ill. Chicago
A scientist measures the standard enthalpy change for the following reaction to be 888.2 kJ : 2NH3(g) + 3 N2O(g) 4N2(g) + 3 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation o

10.5_heating Curves
School: Ill. Chicago
The following information is given for tin at 1atm: boiling point = 2270oC melting point = 232.0oC specific heat solid= 0.2260 J/goC specific heat liquid = 0.2430 J/goC Hvap(2270oC) = 1939 J/g Hfus(232.0oC) = 59.60 J/g A 26.30 g sample of liquid tin at 58

10.5_Enthalpy Rxn From Enthalpy Formation
School: Ill. Chicago
CO(g) + Cl2(g) COCl2(g) Feedback: The standard enthalpy of a reaction may be calculated from the standard heats of formation of the products and the reactants. H o rxn = o H f(products)  o H f(reactants) Moles Species Products 1 COCl2(g) Reactants 1 CO(g

10.5
School: Ill. Chicago
The following information is given for bismuth at 1atm: boiling point = 1627oC melting point = 271oC specific heat solid= 0.126 J/goC specific heat liquid = 0.151 J/goC Hvap(1627oC) = 172 kJ/mol Hfus(271oC) = 11.0 kJ/mol What is H in kJ for the process of

10.5 Phase Changes With Heating.cooling
School: Ill. Chicago
The following information is given for iron at 1atm: boiling point = 2750oC melting point = 1535oC specific heat solid= 0.4520 J/goC specific heat liquid = 0.8240 J/goC Hvap(2750oC) = 6338 J/g Hfus(1535oC) = 289.2 J/g A 25.30 g sample of solid iron is ini

10.5 Part3
School: Ill. Chicago
Identify the line segment on the following diagram where the specific heat of the solid is used to calculate energy flow. line segment AB line segment BD line segment FH line segment HJ line segment DF Feedback: The specific heat is used to calculate

LAB 1 Heat Of Vaporization
School: Ill. Chicago
Wonjung Joanne Han CHEM 114 Section 18665 1/22/13 LAB 1: Heat of Vaporization of Nitrogen Objective In this lab, the energy needed to boil one gram of liquid nitrogen will be determined by letting a known mass of it interact with warm water in a Styrofoam

W2.ans
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11.6_C_1
School: Ill. Chicago
For the reaction 2NO(g) + 2H2(g) N2(g) + 2H2O(l) o o H = 752 kJ and S = 352 J/K At standard conditions, this reaction would be product favored at relatively high temperatures. at no temperature. at all temperatures. at relatively low temperatures. Feedb

CHEM 114  Chap 18__Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 18 1. Determine Lewis structure and formal charges of the following. (Include resonance if present.) NO3 ion , SnCl2 , IF5 2. Based on your Lewis structures above, identify the following for each species above. NO3 ion SnCl2 IF

CHEM 114  Chap 19 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problem Solutions Chapter 19 1) Name the following compounds: [Cu(NH3)4]Cl2 tetraamminecopper(II) chloride (NH4)2[Fe(H2O)Cl5] ammonium aquapentachloroferrate(III) [Co(NH3)6][Cr(CN)6] hexaaminecobalt(III) hexacyanochromate(III) (any consistent set

CHEM 114  Chap 20 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 10 Practice Problem Solutions_Feb 2012
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Su12_Coordination Compounds  Worksheet_July2012
School: Ill. Chicago
Course: Honors General Chemistry II
Chemistry 114 Summer 2012 Practice Group Worksheet on Coordination Compounds The transition metal elements have unique physical and chemical properties owing to the five d orbitals within the (n1) shell to accommodate electrons. One of the more character

CHEM 114  Chap 13 _Practice Problems Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 14_Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 14 1) In the reaction below, suppose d[H2O]/dt is 0.42 molL1min1. 4 NH3(g) + 7 O2(g) 4 NO(g) + 6 H2O(g) Determine the following: a. rate of reaction. b. rate of formation of NO c. rate of change of O2 concentration 2) Given the

CHEM 114  Chap 14 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 17__Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 17 1. Identify the following elements or ions from electron configuration. a. 1s22s22p63s23p4 b. [Ar]3d104s1 c. ion with +2 charge, [Kr]4d6 2. What is the maximum number of electrons that can go in the following shells or subshe

CHEM 114  Chap 17_ Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 10_ Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 10 1) A 5.00 cm3 block of zinc heated to 85.0 0C is submerged into a constant pressure calorimeter containing 100.0 g of water at 25.0 0C. After reaching thermal equilibrium, the final temperature of the water is 26.9 0C. Water h

CHEM 114  Chap 16 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 16__Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 16 Some Useful Constants: Planck's constant h = 6.626 x1034 J s Electron mass me = 9.109 x1031 kg Rydberg constant Ry = 2.180 x1018 J Speed of light in vacuo c0 = 2.998 x108 m s1 Electron charge e = 1.602 x1019 C 1) What is the w

CHEM 114  Chap 15 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Worksheet Chapter 15 1) Calculate the energy released by the fission: 235 92U + 1 0 n 9438Sr + 139 54Xe + 3 10n Given the following atomic masses: 23592U 235.0439 u 9438Sr 93.9154 u , 13954Xe 138.9179 u Mass of neutron = 1.0087 amu. What percent

CHEM 114  Chap 11 Practice Problems Solutions_Feb 2012
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 11 Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chap 11 1) Fill in the blank. ( < , > , = ) a. At equilibrium, the G of reaction _ 0. b. In order for an endothermic reaction to be spontaneous, the change of entropy must be _ 0. c. If G is > 0 then the equilibrium constant, K _ 1. d. E

CHEM 114  Chap 12_Practice Problems Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 13 _Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 13 1) a. For the electrochemical cell, Pt Fe2+, Fe3+  Co2+  Co, the halfreaction occurring at the anode is_. b. One joule per coulomb equal to 1 _. c. A galvanic cell is the same as a voltaic cell. (True or false). d. An elec

CHEM 114  Chap 18 Practice Problem Solutions
School: Ill. Chicago
Course: Honors General Chemistry II

Practice Problems And Exam Review For Constants And Rate Examples
School: Ill. Chicago
Course: College Chemistry II

Math_8_Functions And GraphsLogs And Exponents
School: Ill. Chicago
Laws of Logarithms In order to solve problems or to handle data, it is useful to know several algebraic relationships involving logarithms. Since natural logarithms are most often used in chemistry, the following relationships will be expressed as natural

Math_7_Logarithm Calculations
School: Ill. Chicago
Logarithms The logarithm of a number to a certain base is the power to which the base must be raised to get the number. There are two bases in wide use: base 10 and base e, where e is a number like pi and has the value 2.718. Logarithms to the base e are

11.8_C
School: Ill. Chicago
A student determines the value of the equilibrium constant to be 2.42E25 for the following reaction. CH4(g) + H2O(g) 3H2(g) + CO(g) Based on this value of Keq: o G for this reaction is expected to be (greater,less) than zero. Calculate the free energy ch

11.8_B
School: Ill. Chicago
For the reaction I2(g) + Cl2(g) 2ICl(g) o H = 26.8 kJ and o S = 11.4 J/K The equilibrium constant for this reaction at 337 K is Assume that o H and o S are independent of temperature. Feedback: The equilibrium constant is related to the change in the sta

11.7_The Reaction QuotientA
School: Ill. Chicago
The Reaction Quotient The reaction quotient, Q, tells if a reaction is at equilibrium. It has the identical form as the equilibrium constant, K, but the concentrations used are not necessarily the equilibrium concentrations. For a general reaction: aA + b

11.7_LeChatelier
School: Ill. Chicago
LeChatelier's Principle: A change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner as to reduce or counteract the effect of the change. Factors that determine the equilibrium cond

11.7_Free Energy For Nonstandard Concentrations
School: Ill. Chicago
Consider the reaction CO(g) + Cl2(g) COCl2(g) Use the standard thermodynamic data in the tables linked above. Calculate G for this reaction at 298.15K if the pressure of COCl2(g) is reduced to 17.57 mm Hg, while the pressures of CO(g) and Cl2(g)remain at

11.7_7B_Reaction Quotient
School: Ill. Chicago
Consider the following reaction where Kc = 154 at 298 K: 2 NO(g) + Br2(g) 2 NOBr(g) A reaction mixture was found to contain 5.34E2 moles of NO(g), 4.23E2 moles of Br2(g) and9.85E2 moles of NOBr(g), in a 1.00 Liter container. Is the reaction at equilibr

11.7_4c_Equilibrium
School: Ill. Chicago
Write the equilibrium constant expression, Kc, for the following reaction: Please enter the compounds in the order given in the reaction. If either the numerator or denominator is 1, please enter 1 NH3(g) + H2S(g) NH4HS(s) Feedback: The equilibrium consta

11.7.11c_LeChatelier's Principle  Concentration
School: Ill. Chicago
LeChatelier's Principle: A change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner as to reduce or counteract the effect of the change. Factors that determine the equilibrium cond

Review Worksheet Exam Two Topics  Rate Of Constant And Initial Concentration
School: Ill. Chicago
Course: College Chemistry II

CHEM 114  Coordination Compound Worksheet Key_Su12
School: Ill. Chicago
Course: Honors General Chemistry II

CHEM 114  Chap 12__Practice Problems
School: Ill. Chicago
Course: Honors General Chemistry II
Practice Problems Chapter 12 1) Balance the following redox reactions in acidic aqueous solution by halfreaction method. BrO3(aq) + N2H4(g) Br(aq) + N2(g) MnO4(aq) + Al(s) Mn2+(aq) + Al3+(aq) SO32(aq) + MnO4(aq) SO42(aq) + Mn2+(aq) 2) Balance the f