CALORIMETRY Abstract: During the experiment‚ the group were able to perform the following objectives; to compute the heat capacity of a Styrofoam-cup calorimeter‚ and also to compute the heat of neutralization of 1.0 M hydrochloric acid and 1.0 M sodium hydroxide‚ the heat of dilution of concentrated sulfuric acid‚ and the heat of solution of solid ammonium chloride The sixth experiment was named "Calorimetry" wherein it is the measurement of how much heat is gained or released by a system
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19.53a‚ 19.55‚ 19.61‚ 19.73‚ 19.75‚ 19.77 Recall from Chapter 5 - 1st Law of Thermodynamics o Energy is neither ____________________________________________. o Energy of the universe is constant. o Enthalpy Change ▪ Heat energy transferred at _____________________________________ ▪ Negative value = ▪ Positive value = Spontaneous Processes - Thermodynamics o Tells us the _______________________________________
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Chapter 15 (not much on E) Thermodynamics: Enthalpy‚ Entropy & Gibbs Free Energy Thermo 2 Thermodynamics: thermo = heat (energy) dynamics = movement‚ motion Some thermodynamic terms chemists use: System: the portion of the universe that we are considering open system: energy & matter can transfer closed system: energy transfers only isolated system: no transfers Surroundings: everything else besides the system Isothermal: a system that is kept at a constant temperature
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Eng. Programme‚ KM21102. SEMS-1-2011/2012 Lecture 6. Tue. 15 / 10/ 2012 Lecture Room DKP 10 Engineering Thermodynamics Lecture 6: Evaluating Properties Using the Ideal gas OUTLINE: Real gases‚ specific heats‚ internal energy‚ enthalpy In this section the ideal gas model is introduced. The ideal gas model has many applications in engineering practice and is frequently used in subsequent section of this text. Ideal gas Equation state From the Generalized compressibility
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Borate. Alexis Cervantes and Ak Young. CHEM 114-07 April 30‚ 2024. Introduction The purpose of this experiment was to evaluate thermodynamic values and understand their relationship to equilibrium constants. By measuring the change in enthalpy (H°) and the change in entropy (S°)‚ the equilibrium constant (Ksp) was determined for the dissolution of borax in water. In procedure one of the experiment‚ the temperature of the borax solution was varied and its saturation level was measured at
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Course Name Fundamentals in Chemistry Course Code: CHEM 101 Course Provider: The Division of Arts‚ Sciences and General Studies Level 1 Semester in which course is offered: 1 No. of Credits: 4 Total Study Hours: 56 Course Description: This course introduces students to the fundamental concepts in chemistry. It explores the structure of the atom‚ bonding between atoms/particles‚ the concept of the mole‚ redox reactions‚ kinetic theory and energetics. A laboratory component will be
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SEPERATING CYCLOHEXANE AND TOLUENE BY DISTILLATION Aim: Separate two miscible liquids‚ either by macroscale or microscale process‚ using simple and fractional distillation. Compare the efficiencies of simple and fractional distillation. INTRODUCTION: The purpose of this experiment is to learn how to separate two miscible liquids by microscale process. There will be use of simple and fractional distillation. Simple and fractional distillation efficiencies will be compared. The student should have
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Data collection Quantitative Data Raw Data Table 1: Table showing the mass of the amount of unknown acid X measured in grams (±0.001g) Table 2: Table of reading of the burette initially filled with 25mL of 0.201moldm-3 sodium hydroxide (NaOH) to titrate 25mL (±0.03mL) of unknown acid X in mL (±0.05mL) after each titre. Reading on the burette initially filled with 25mL of 0.201moldm-3 NaOH (±0.05mL) First titre 21.3 Second titre 18.2 Third titre 15.2 Fourth titre 12.0 Qualitative
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Question: What is the molar concentration of acetic acid in a sample of vinegar? Prediction: The manufacture of claims on the label that the vinegar contains 5.0% acetic acid‚ which translates into a 0.87 mol/L concentration of acetic acid. The concentration of acetic acid in the vinegar sample should be the same. Purpose: If we add acid solution to basic solution to produce water and salt this activity is called titration. It involves carefully adding one solution to another until chemically
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titration is a titration technique where the endpoints of the reaction are located from the enthalpy change between the reagents. In thermometric titration we make use of the fact that reactions in solution are accompanied by temperature changes and thus it is possible to follow the course of the reaction with a thermometer. A reagent of known concentration is added to the reagent of unknown concentration and the enthalpy changes presented on a graph to show the endpoint and maximum and minimum temperatures
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