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CHEM 114 - Ill. Chicago Study Resources
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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

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• 5) Electrochemical Measurement and Batteries (1)
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5) Electrochemical Measurement And Batteries (1)

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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

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The Slope

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The slope-intercept 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 (y-axis) against x (x-axis): A straight line can be represented in the form y = mx + b where b =

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OWL-algebra

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

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• Heat Capacity Definitions-chapter 10.1
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Heat Capacity Definitions-chapter 10.1

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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

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Heat Capacity Definitions-3

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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

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Heat Capacity Definitions-2

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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

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Heat Capacity Definitions-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

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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

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Exponent Algebra Rules

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

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Energy Unit Conversions

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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

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Direct And Inverse Proportions

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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

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Calorimetry_Q1

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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

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• 11.2_ Entropy Change for a Reaction
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11.2_ Entropy Change For A Reaction

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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

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11.7_4c_Equilibrium

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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

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• 11.7.11c_LeChatelier's Principle - Concentration
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11.7.11c_LeChatelier's Principle - Concentration

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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

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11.6_C_2

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For the reaction 2H2O(l) 2H2(g) + O2(g) o o H = 572 kJ and S = 327 J/K o G would be negative at temperatures (above, below) K. Enter above or below in the first box and enter the temperature in the second box. Assume that o H and o S are constant. Feedbac

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11.6_C_1

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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

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• 11.5_C_GibbsHelmholtz Equation Calculations
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11.5_C_GibbsHelmholtz Equation Calculations

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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

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11.5_C_3Qualitative Delta G, H, S

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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

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• 11.5_C_2delta Go rxn from formation data
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11.5_C_2delta Go Rxn From Formation Data

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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

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11.4

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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

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11.3_Entropy And The Second Law

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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

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• 11.3_B_Favored from delta So universe calculation
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11.3_B_Favored From Delta So Universe Calculation

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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

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11.2_a_balance Half Rxns

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Balancing Oxidation-Reduction 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

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Calorimetry Hw3

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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

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Calorimetry Hw2

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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

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Calorimetry Hw1

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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

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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

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W5.ans

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Graph 3

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Graph 4

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GRAPH 2

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GRAPH 1

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EMISSION SPECTRA!

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Theemissionspectraofsomeelements INTRODUCTION: thepurposeofthislabistoobservethespectraofdifferentemissionsourcesusinga gratingspectrometerandusespectrometertoidentifytheunknown,Therewillbeasetofunknownsforeach labsection.Wewillalsocalculatetheenergyleve

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6)

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time 5 10 15 20 25 30 35 40 45 50 [CrO3Cl-] 2.04E-03 2.14E-03 2.02E-03 1.86E-03 1.78E-03 1.53E-03 1.55E-03 1.51E-03 1.44E-03 1.34E-03 [CrO3Cl-]^2 4.16E-06 4.58E-06 4.08E-06 3.46E-06 3.17E-06 2.34E-06 2.40E-06 2.28E-06 2.07E-06 1.80E-06 5.00E-06 f(x) = 1.0

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2) Calorimetry And Hess's Law

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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

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• 6) The Rate of the Oxidation of Ethanol by Chromium(VI) (1)
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6) The Rate Of The Oxidation Of Ethanol By Chromium(VI) (1)

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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

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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 A-B line segment B-D line segment F-H line segment H-J line segment D-F Feedback: The specific heat is used to calculate

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• 10.5 phase changes with heating.cooling
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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

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10.5

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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

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Assignment List

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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

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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

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• 10.7_Bond Enthalpy from Enthalpy Rxn
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10.7_Bond Enthalpy From Enthalpy Rxn

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The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol Feedback: Given the enthalpy of a gas phase reaction, the N-H bond energy may be estimated by taking int

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10.6-Enthalpy And Hess's Law

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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 =?

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• 10.6_Enthalpy Formation from Enthalpy Rxn
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10.6_Enthalpy Formation From Enthalpy Rxn

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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

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10.5_heating Curves

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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

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• 10.5_Enthalpy Rxn from Enthalpy Formation
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10.5_Enthalpy Rxn From Enthalpy Formation

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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

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Theoretical Wavelengths

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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

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11.7_7B_Reaction Quotient

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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 5.34E-2 moles of NO(g), 4.23E-2 moles of Br2(g) and9.85E-2 moles of NOBr(g), in a 1.00 Liter container. Is the reaction at equilibr

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• organic-2-organic-chemistry-klein-70-ch-7-substitution-reactions-2636
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Organic-2-organic-chemistry-klein-70-ch-7-substitution-reactions-2636

School: Ill. Chicago

Course: Honors General Chemistry II

ORGANIC - KLEIN 2E CH.7 - SUBSTITUTION REACTIONS ! ! www.clutchprep.com ORGANIC - KLEIN 2E CH.7 - SUBSTITUTION REACTIONS CONCEPT: INTRODUCTION TO SUBSTITUTION Previously, we discussed the various ways that acids could react with bases: Recall that in the

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• CHEM 114 - Chap 13 _Practice Problems
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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 half-reaction 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

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• CHEM 114 - Chap 14_Practice Problems
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CHEM 114 - Chap 14_Practice Problems

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Course: Honors General Chemistry II

Practice Problems Chapter 14 1) In the reaction below, suppose d[H2O]/dt is 0.42 molL-1min-1. 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

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• CHEM 114 - Chap 13 _Practice Problems Solutions
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CHEM 114 - Chap 13 _Practice Problems Solutions

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 19 Practice Problem Solutions
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CHEM 114 - Chap 19 Practice Problem Solutions

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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

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CHEM 114 - Quiz 3 With Answers

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Course: Honors General Chemistry II

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CHEM 114 - Quiz 4 With Answers

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 20 Practice Problem Solutions
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CHEM 114 - Chap 20 Practice Problem Solutions

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Course: Honors General Chemistry II

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CHEM 114 - Quiz 4 Answer Keys

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Course: Honors General Chemistry II

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CHEM 114 - Quiz 2 Answer Key

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 10 Practice Problem Solutions_Feb 2012
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CHEM 114 - Chap 10 Practice Problem Solutions_Feb 2012

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Course: Honors General Chemistry II

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• CHEM 114 - Su12_Coordination Compounds - Worksheet_July2012
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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 (n-1) shell to accommodate electrons. One of the more character

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• CHEM 114 - Chap 12_Practice Problems Solutions
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CHEM 114 - Chap 12_Practice Problems Solutions

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 11 Practice Problems
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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

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• CHEM 114 - Chap 11 Practice Problems Solutions_Feb 2012
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CHEM 114 - Chap 11 Practice Problems Solutions_Feb 2012

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Course: Honors General Chemistry II

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Chemlabs114

School: Ill. Chicago

Course: Honors General Chemistry II

Time Volume 0 0.5 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.0 9.0 0.4 (mm) Millimoles millimoles 0 0.017 0.034 0.071 0.095 0.174 0.215 0.234 0.282 0.315 0.355 0 0.672 1.34 2.80 3.75 6.87 8.49 9.24 11.14 12.44 14.02 Experiment 1 f(x) = 0.0404051522x - 0.0042213115 R =

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Chem Lab Experiment Two

School: Ill. Chicago

Course: Honors General Chemistry II

A) Indipendent^ Y- axis mass balance reading Deviation Abs. val % dev 0.10 0.09650 -0.00350 0.0035 0.350 0.50 0.48920 -0.01080 0.0108 1.080 1.00 1.01250 0.01250 0.0125 1.250 2.00 2.01850 0.01850 0.0185 1.850 5.00 5.02500 0.02500 0.025 2.500 Dependent^ Mas

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Thermodynamics

School: Ill. Chicago

Course: Honors General Chemistry II

1.Estimate the value of the equilibrium constant at 550 K for each of the following reactions. A) 2CO(g)+O2(g)2CO2(g) K=_ B) 2H2S(g)2H2(g)+S2(g) K=_ 2. A reaction has an equilibrium constant of 6.610 3at 298 K. At 730K , the equilibrium constant is 0.77.

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• CHEM 114 - Chap 18__Practice Problems
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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

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• CHEM 114 - Chap 14 Practice Problem Solutions
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CHEM 114 - Chap 14 Practice Problem Solutions

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 17__Practice Problems
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CHEM 114 - Chap 17__Practice Problems

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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 sub-she

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• CHEM 114 - Chap 17_ Practice Problem Solutions
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CHEM 114 - Chap 17_ Practice Problem Solutions

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 10_ Practice Problems
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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

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• CHEM 114 - Chap 16 Practice Problem Solutions
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CHEM 114 - Chap 16 Practice Problem Solutions

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Course: Honors General Chemistry II

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• CHEM 114 - Chap 16__Practice Problems
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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

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• CHEM 114 - Chap 15 Practice Problem Solutions
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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

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CHEM 114 - Quiz 3__Key

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Course: Honors General Chemistry II

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CHEM 114 - Quiz 2 With Answers

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Course: Honors General Chemistry II

• 4 Pages
• The H Atom and Quantum Mechanics Intermediate Discusion
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The H Atom And Quantum Mechanics Intermediate Discusion

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Course: College Chemistry II

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• Worksheet on Quantum Numbers and Energy shells
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Worksheet On Quantum Numbers And Energy Shells

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Course: College Chemistry II

• 11 Pages
• Review Worksheet Exam Two Topics - Rate of Constant and Initial Concentration
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Review Worksheet Exam Two Topics - Rate Of Constant And Initial Concentration

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Course: College Chemistry II

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• Worksheet Rates Laws and Nernst Equation
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Worksheet Rates Laws And Nernst Equation

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Course: College Chemistry II

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• Practice Problems and Exam Review for Constants and Rate Examples
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Practice Problems And Exam Review For Constants And Rate Examples

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Course: College Chemistry II

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• Math_8_Functions and GraphsLogs and Exponents
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Math_8_Functions And GraphsLogs And Exponents

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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

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Math_7_Logarithm Calculations

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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

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11.8_C

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A student determines the value of the equilibrium constant to be 2.42E-25 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

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11.8_B

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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

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11.7_The Reaction QuotientA

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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

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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

• 4 Pages
• Review Worksheets and Notes on Atomic Configuration
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Review Worksheets And Notes On Atomic Configuration

School: Ill. Chicago

Course: College Chemistry II

• 6 Pages
• Electrolysis and Galvanic and Electrolytic Cells
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Electrolysis And Galvanic And Electrolytic Cells

School: Ill. Chicago

Course: College Chemistry II

• 4 Pages
• WkShop on Linear Regression Analysis and Volume
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WkShop On Linear Regression Analysis And Volume

School: Ill. Chicago

Course: College Chemistry II

• 12 Pages
CHEM 114 - Quiz 1 Answer Key

School: Ill. Chicago

Course: Honors General Chemistry II

• 5 Pages
• CHEM 114 - Chap 18 Practice Problem Solutions
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CHEM 114 - Chap 18 Practice Problem Solutions

School: Ill. Chicago

Course: Honors General Chemistry II

• 12 Pages
CHEM 114 - Practical 3_Quizzes A_D

School: Ill. Chicago

Course: Honors General Chemistry II

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