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    GCII Lab 1

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    Experiment I: Thermochemistry Background: Thermochemistry is the branch of chemistry that focuses on the studies of chemical reactions or physical changes and heat associated with chemical reactions. According to the first law of thermodynamics‚ energy cannot be created or destroyed but it can be converted from one form into another and/or transferred between different atoms‚ molecules‚ or substances. In general‚ energy can be classified into two categories: kinetic and potential. Kinetic energy

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    religion

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    (KJ/mole) Number of Bonds Total (KJ/mole) C-H 412 7 2884 C=O 802 6 4812 C-C 348 2 696 H-O 463 8 3704 O=O 496 5 2480 C-O 366 1 366 O-H 463 1 463 Total 6889 Total 8516 Table 5: Shows the theoretical heat change in enthalpy for Propanol From the above results‚ the theoretical change in enthalpy can be calculated. The following calculation is done by Hess’s law: ∆H=∑Energy of broken bonds-∑Energy of bonds made=6889-8516= -1627 KJ/MoleExperimental Heat of Reaction: Energy Produced: q=mC∆T=100 ×4.18 ×14q=5852JEnergy

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    Anythings

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    endothermic change. For example‚ cold packs used to relieve swelling joints or muscles often use chemicals that absorb heat when mixed‚ so the packs feel cold. When a reaction is carried out under constant pressure‚ the heat of a reaction is defined as the enthalpy change for the reaction (ΔH). Since most reactions occur under constant atmospheric pressure‚ the heat of a reaction is equal to ΔH‚ which is generally reported in units of kilojoules (kJ) per mole of the reactants and products as shown in the balanced

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    Labreport Solubility

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    molarities. Then‚ the equilibrium constant was calculated and a graphical relationship between the natural logarithm of the equilibrium constant and the inverse of the temperature gave a linear plot that allowed the determination of Gibbs free energy and enthalpy changes associated with the reaction. From there‚ the entropy change associated with the reaction was determined. PROCEDURE: 1. Weigh out 20.0g of potassium nitrate and transfer it to a 25x200mL test tube. Do not ingest the potassium nitrate

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    Deicer Magnesium Chloride

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    as a road salt. The Van’t Hoff factor of the salt and the enthalpy of dissolution when dissolved in pure water were experimentally tested to evaluate its many characteristics as a deicer. To determine the Van’t Hoff factor‚ the difference of temperatures of freezing water and a solution of magnesium chloride was determined. A Van’t Hoff factor average of 2.88 was found‚ which is close to the ideal Van’t Hoff factor value of 3. The enthalpy of dissolution was found using calorimetry. Various amounts

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    dissolving in the water absorb energy from the surroundings and the measured temperature of the surroundings (beaker‚ air) drops. 2. The phase change from a gas to a liquid is called condensation. Is the enthalpy change‚ g → l‚ exothermic or endothermic? Explain. The enthalpy change is exothermic. Recall that energy is always released when new bonds form. Here‚ the phase change involves the formation of intermolecular attractions releasing energy as the particles adopt lower-energy

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    entropy book

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    5.2.2 Enthalpy and Entropy For 2013-2014 S for melting vs. boiling Discuss How do chemists work out whether a reaction will happen or not? There are various ways including equilibrium constants‚ standard electrode potentials and enthalpy values. But how are these related? There is a more fundamental concept which links all these together. Remember? Enthalpy is a measure of heat energy and ΔH is the enthalpy change which we studied at AS. Questions 1. Which sign for ΔH would

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    Thermodynamics Lab Report

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    including enthalpy of reaction‚ heat of formation‚ Hess’s Law‚ and calorimetry. The enthalpy of reaction‚ ΔHrxn is the heat or enthalpy change for a chemical reaction. The energy change is equal to the amount of heat transferred at a constant pressure in the reaction. The change represents the difference in enthalpy of the products and the reactants and is independent of the steps in going from reactants from products. The heat of formation (ΔH°f)‚ which is also known as standard enthalpy of formation

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    absorbs heat. Enthalpy of reaction : The change in internal energy (H) through a reaction is △H. 6.1.3 △H will be negative for exothermic reactions (because internal heat is being lost) and positive for endothermic reactions (because internal energy is being gained). 6.1.4 The most stable state is where all energy has been released. Therefore when going to a more stable state‚ energy will be released‚ and when going to a less stable state‚ energy will be gained. On an enthalpy level diagram‚

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    Alcohol Combustion Plan

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    Comparing the enthalpy changes of combustion of different alcohols Aim In this experiment I will investigate the enthalpy changes of combustion. In particular I will be investigating the enthalpy change of combustion for different alcohols. I hope to investigate some of the homologous series alcohols‚ as well as a few structural isomers of these alcohols. Background & theory Enthalpy cannot be measured. What we can actually measure is the enthalpy change from the reactants to the products.

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