CHEM 104: General Chemistry II Spring 2014 Exam 1 Version A Instructions: 1. Do NOT open this exam until you are told to do so. Opening the exam before the start of the exam is considered an act of Academic Dishonesty. 2. All answers must be bubbled into the scantron answer sheet. 3. No credit will be given for answers written on this exam. 4. You must use a #2 pencil to bubble in the answers on your scantron. 5. This is a multiple choice exam consisting of 30 questions (7 pages). Each question
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F UNDAMENTALS OF T HERMODYNAMICS SEVENTH EDITION CLAUS BORGNAKKE RICHARD E. SONNTAG University of Michigan John Wiley & Sons‚ Inc. PUBLISHER ASSOCIATE PUBLISHER ACQUISITIONS EDITOR SENIOR PRODUCTION EDITOR MARKETING MANAGER CREATIVE DIRECTOR DESIGNER PRODUCTION MANAGEMENT SERVICES EDITORIAL ASSISTANT MEDIA EDITOR COVER PHOTO Don Fowley Dan Sayre Michael McDonald Nicole Repasky Christopher Ruel Harry Nolan Hope Miller Aptara® Corporation Inc. Rachael Leblond Lauren Sapira c Corbis Digital
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on heating times. Process Parameters The process parameters and initial conditions for Example 1 are given in the table below. (initial bulk liquid temperature) 27.2 C (heat capacity) 2.516 kJ/kg K (mass of bulk liquid in vessel) 329 kg (heat capacity) 1.65 kJ/kg K (initial guess) 257 W/K Jacket flow rate 5 kg/s Model Summary DynoChem provides several utilities for characterizing vessels. These include a template for fitting heat transfer coefficients
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investigation of the Dissolution of Solutes Background Information Molar heat of solution * The molar heat of solution of a substance is the heat absorbed when one mole of the substance dissolves in a large excess of water. It is expressed in kJ/mol. * The specific heat of water is a constant‚ with a value of 4.18 J/ g*oC. AIM: To determine the molar heat of solution for two different solids Equipment: * A calorimeter (made using 2 Styrofoam cups with a cardboard lid) * Electronic
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Abstract: This report is a description of an experimental determination of the enthalpy of reaction of sulfuric acid in a reaction with magnesium to produce magnesium sulfate. Through the use of an ice calorimeter‚ the rxn H° D for this reaction is determined to be 1 360kJ mol − − × . Introduction: This report details an experiment in thermochemistry. Included are the methods‚ results‚ and interpretation of results of an experimental determination of an enthalpy of reaction. The reaction
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• The equilibrium law DYNAMIC EQUILIBRIUM forward A +8 reaction ""r=====~’~ reverse reaction Most chemical reactions do not go to completion. Once some products are formed the reverse reaction can take place to reform the reactants. In a closed system the concentrations of all the reactants and products will eventually become constant. Such a system is said to be in a state of dynamic equilibrium. The forward and reverse reactions continue to occur‚ but at equilibrium
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7/16/12 Heat of Fusion Heat of Fusion for Ice Introduction: This lab report is a step by step process in calculating the heat of fusion for ice and to compare the differences between salt added to room temperature water and salt added to icy water. To calculate heat of fusion‚ one must understand heat of fusion. Heat of fusion is the amount of heat required to convert a mass of a solid at its melting point into a liquid without an increase in temperature. As difficult as this may sound‚
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Individual Assignment. Each student is required to complete the task in a full handwriting on an A4 paper. Due Date of Submission on 30th November 2011‚ before 2.00 PM. Late submissions will not be entertained. 1. A 1.8-m rigid tank contains steam at 220°C. One third of the volume is in the liquid phase and the rest is in the vapor form. Determine (a) the pressure of the steam‚ (b) the quality of the saturated mixture‚ and (c) the density of the mixture. 3 2. A piston–cylinder device contains
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Joseph Corey‚ Chris‚ Grant Thermodynamics – Enthalpy of Reaction and Hess’s Law I. Purpose The purpose of this lab is to verify Hess’s Law through the three reactions of NaOH and HCl‚ NH4Cl and NaOH‚ and NH3 and HCl. The sum of the enthalpies of the first two reactions should equal the enthalpy of the third reaction. II. Background Hess’s Law is used to determine the enthalpy of a reaction from adding two or more preceding reactions. To determine the enthalpies of certain
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recording the change in temperature with a temperature probe; and calculate the enthalpy of reaction from the data found. The specific heat capacity was found to be and average of 20.0 J/(g(°C)). The enthalpy of the reaction was found to be -64.5 kJ/mol. These values show that the specific heat of the calorimeter is nearly unimportant when calculating the enthalpy when compared to other data. Introduction The purposes of this experimentation was to determine the specific heat capacity constant
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