"Molar enthalpy of neutralization" Essays and Research Papers

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    Hess’ Law of Heat Summation Hess’ Law states that: "The enthalpy change for any reaction depends  on the products and reactants and is independent  of the pathway or the number of steps between  the reactant and product".  BASICALLY:    Hess’ Law states "the heat evolved or absorbed in     a chemical process is the same whether the process     takes place in one or in several steps"     ­­>This is also known as the "law of constant heat summation".       All it means is that no matter how many steps the chemical 

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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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    = 23.2 ˚C Enthalpy change: Now using all the variables obtained we can calculate the enthalpy change for the reaction using (∆H) = mc∆T Now‚ Mass of copper (II) sulfate (CuSO_4) = 25 〖cm〗^3 Temperature change (∆T) = 23.2 ˚C Specific heat capacity of water = 4.18 J g-1 k-1 Using the equation provided above‚ we can plug in the values necessary to find the enthalpy change (∆H) = 25 〖cm〗^3 X 23.2 ˚C X 4.18 J g-1 k-1 (∆H) = - 2424.4 J Now to find the enthalpy change per mole or (kJ/Mol)

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    06.03 Calorimetry: Lab Report Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page. Part I The Dissolving of Solid Sodium Hydroxide in Water Procedure: 1. Measure out approximately 200 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table.

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    HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers |Chapter 25 Simple molecular substances with non-octet |Page Number | |structures and shapes of simple molecules | | |Class Practice |1 | |Chapter Exercise

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    called a calorimeter‚ an insulating container that minimizes heat exchange between its contents and the surrounding. Heat flow in a device called a calorimeter. In this experiment‚ we should find the heat capacity of the calorimeter‚ the heat of neutralization and the specific heat of a metal. Data: A. Specific Heat Trial 1 Trial 2 Trial 3 Mass of stoppered test tube 5.2g 5.2g 5.2g Mass of stoppered test tube and metal 8.7g 8.7g 8.7g Mass of calorimeter 4.9g 4.9g 4.9g

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    -(ΔHwater * nLR) / ΔT (eq 1) where ΔHwater is the enthalpy change of water. This is equal to -55.81 kJ/mol. nLR is the number of moles of the limiting reactant‚ and ΔT is the change in temperature associated with the reaction. The Ccal obtained was later used to determine the experimental values of the enthalpy change of the reactions (ΔHrxn). Six other reactions were also used to determine its enthalpy change. The reactions are: Neutralization: a. Ammonia and hydrochloric acid (NH3(aq)

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    Chapter 34 Importance of redox reactions in modern ways of living Class Practice 36 Chapter Exercise 37 Part Exercise 39 Chapter 35 Energy changes in chemical reactions Class Practice 42 Chapter Exercise 43 Chapter 36 Standard enthalpy change of combustion‚ neutralization‚ solution and formation Class Practice 44 Chapter Exercise 46 Chapter 37 Hess’s Law Class Practice 48 Chapter Exercise 51 Part Exercise 53 Chapter 25 Simple molecular substances with non-octet structures and shapes of simple molecules

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    Calorimetry Experiment Purpose: The objective of this lab is to determine the enthalpy change for NaOH(aq) + HCl(aq) NaCl (aq) + H2O(l) Procedure: Before measuring the enthalpy of acid base neutralization‚ my partner Brian and I determined a calorimeter constant‚ using a homemade polystyrene calorimeter. With the following formula and data: qhot= cm (Tf-Ti) qcold=cm(Tf-Ti) SYSTEM DATA SURROUNDINGS DATA Water cold Mass: 50mL Water hot Mass: 50mL C=4.18 C=4.18 Ti=20 C Ti=31

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    Heat of Mixing: Ethanol and Water Abstract The temperature change when known amounts of water and ethanol were mixed was determined to see the enthalpy change in an isothermal and isobaric environment. Agreeable data was found compared to similar experiments. As the mole fraction increased of the solution so did the enthalpy until a certain limit of about 0.32. Since water’s structure and unique properties affect many aspects of a solution‚ the solutions enthalpy’s decreased at a certain time

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