Data TableInitialChange inTemperature(°C)ReactionMass ofFinal%23solution (g)Temperature(°C)Temperature(°C)502530.305.302502536.9711.973502531.676.67Processing Data1. Calculate the heat energy released for each reaction. Show all your work.Reaction 1:Reaction 2:Reaction 3:2. Write net ionic equations for Reactions 1, 2 and 3. Consider the heat given off inyour reactions; include the heat evolved in kJ/mole for each reaction.Reaction1:Reaction 2:Reaction 3:3. The energy in Reaction 1 represents the energy of solution for one mole of NaOH(s). Look at the net ionic equations for Reactions 2 and 3, and make a similarstatement concerning the significance of AH for reactions 2 and 3.4. Apply Hess's Law using the sum of reaction 1 and reaction 3 to find theexperimental value of AH for reactions 2. Show your work below.5. Calculate the percent error between the value of AH for reaction 2 and the sum ofAH for reaction 1 plus AH for reaction 3. (Assume AH for reaction 2 to be theaccepted value). Show your work. Account for any similarity or difference.6. Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would havebeen the number of Joules released in the reaction? What effect would this haveon the value of AH for reaction 1? INTRODUCTION:In this experiment, you will determine and compare the quantity of heat energy releasedin three exothermic chemical reactions.O Reaction 1: Solid sodium hydroxide dissolves in water to form an aqueous solutionof ions.O Reaction 2: Solid sodium hydroxide reacts with an aqueous solution of hydrogenchloride to form water and an aqueous solution of sodium chloride.O Reaction 3: An aqueous solution of sodium hydroxide reacts with an aqueoussolution of hydrogen chloride to form water and an aqueous solution of sodiumchloride.In order to accurately measure the heat released in each reaction, we will be using acalorimeter (for this experiment a Styrofoam cup will act as the calorimeter). The changein temperature that occurs for each reaction will be used to calculate the energy releasedin kilojoules per mole of sodium hydroxide used. We can assume for our calculations thatany heat transferred to the Styrofoam and surrounding air will be negligible. We can alsoassume that the specific heat of any aqueous solution is 4.18 J/g °C.PROCEDURE:Simulation Link: http://chemcollective.org/vlab/138A. Reaction 11. In the glassware menu, take out a 50 mL graduated cylinder and a foam cup. Fromthe instruments menu, take out of the scale. From the chemical stockroom, movethe distilled water and solid NaOH on to the workbench.2. Transfer 50.0 mL of water to the foam cup. To do this, drag the container of wateron the graduated cylinder. (Before you release the mouse button, the cylinder willturn blue to indicate that it is the recipient). A transfer text-bar will activate at thebottom of the screen. Enter "50.0" (ml) and click on pour. (You will notice that thegraduated cylinder reads 50.0 mL).3. Weigh about 1 gram of solid sodium hydroxide pellets, NaOH(s), directly into thefoam cup and record its mass to the nearest 0.01 gram. To do this, place the foamcup on the balance so it registers a mass, then click the "Tare" button. Drag theNaOH bottle onto then foam cup. (When you release the mouse, the bottle will betipped to show that it is in pour mode). Next, type "1.00" (grams) into the transferbar and then click pour. Note that the balance now reads the mass of thetransferred NaOH. You may now take the cup off of the scale and remove the scalefrom the workbench.4. Click on the graduated cylinder and record its temperature.5. Drag the graduated cylinder onto the foam cup. (When you release the mouse, thegraduated cylinder will be tipped to show that it is in pour mode.) Enter "50.0" inthe transfer bar and then click pour.6. Record the highest temperature.7. Remove all equipment from the laboratory bench.B. Reaction 21. Take the 0.5 M HCI from the strong acids cabinet, a new foam cup, and a 50 mLgraduated cylinder from the glassware menu and place them on the workbench.2. Transfer 50.0 mL of 0.50 M hydrochloric acid solution to the graduated cylinder inplace of the water.3. After measuring 50.0 mL of the HCI solution into the graduated cylinder, proceedas before with steps 3 to 6 of the procedure followed for Reaction 1.4. Record the highest temperature.5. Remove all equipment from the laboratory bench.C. Reaction 31. Take out another graduated cylinder, a fresh foam cup, the 1.0 M HCI and 1.0 MNaOH.2. Measure 25.0 mL of 1.0 M hydrochloric acid solution using the graduated cylinderand pour into the foam cup.3. Pour an equal volume of 1.0 M sodium hydroxide solution in the clean graduatedcylinder.4. Record the temperature of each solution to the nearest 0.1°C.5. Pour the sodium hydroxide solution into the foam cup and record the highesttemperature obtained during the reaction.

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Data Table Initial Final Change in Temperature (°C) 5.30 Reaction Mass of # solution (g) Temperature (°C) 25 Temperature (°C) 30.30 1 50 50 25 36.97 11.97 3 50 25 31.67 6.67 Processing Data 1. Calculate the heat energy released for each reaction. Show all your work.

Data Table Initial Final Change in Temperature (°C) 5.30 Reaction Mass of # solution (g) Temperature (°C) 25 Temperature (°C) 30.30 1 50 50 25 36.97 11.97 3 50 25 31.67 6.67 Processing Data 1. Calculate the heat energy released for each reaction. Show all your work.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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