13_Enthalpy_Gen - Experiment Determining the Enthalpy of a...

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Advanced Chemistry with Vernier13 - 1Experiment13Determining the Enthalpyof a Chemical ReactionAll chemical reactions involve an exchange of heat energy; therefore, it is tempting to plan tofollow a reaction by measuring the enthalpy change (∆H). However, it is often not possible todirectly measure the heat energy change of the reactants and products (the system). We canmeasure the heat change that occurs in the surroundings by monitoring temperature changes. Ifwe conduct a reaction between two substances in aqueous solution, then the enthalpy of thereaction can be indirectly calculated with the following equation.q=CpmTThe termqrepresents the heat energy that is gained or lost.Cpis the specific heat of water,misthe mass of water, and ∆Tis the temperature change of the reaction mixture. The specific heatand mass of water are used because water will either gain or lose heat energy in a reaction thatoccurs in aqueous solution. Furthermore, according to a principle known as Hess’s law, theenthalpy changes of a series of reactions can be combined to calculate the enthalpy change of areaction that is the sum of the components of the series.In this experiment, you will measure the temperature change of two reactions, and use Hess’slaw to determine the enthalpy change, ΔHof a third reaction. You will use a Styrofoam cupnested in a beaker as a calorimeter, as shown in Figure 1. For purposes of this experiment, youmay assume that the heat loss to the calorimeter and the surrounding air is negligible.

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Chapter 11 / Exercise 118
Chemistry: The Molecular Science
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The document you are viewing contains questions related to this textbook.
Chemistry: The Molecular Science
The document you are viewing contains questions related to this textbook.
Chapter 11 / Exercise 118
Chemistry: The Molecular Science
Moore/Stanitski
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