Calculate the mass of the reaction mixture in each reaction. (To do this, first determine the total volume of the solution. Then calculate the mass of the solution, based on the assumption that the added solid does not change the volume and that the density of the solution is the same as that of pure water, 1.0 g/mL.) Remember to add the mass of the solid. a) Calculate the total heat released in each reaction, in J, assuming that the specific heat capacity of the solution is the same as that of pure water, 4.184 J/ºC g. Remember: heat of reaction = m C Δ T b) Calculate the number of moles of NaOH used in reactions 1 c) Calculate the number of moles of NaOH used in reaction 3 by multiplying the volume of NaOH times the molarity (1.000 mol/L). d)Calculate the energy released, in kJ/mol, of NaOH for each reaction. Reaction 12. There will be a bottle of NaOH near the balance. A weigh paper will be on the balance withapproximately 4 g NaOH on the paper. Record the mass of NaOH in the data table on thefollowing page.3. The calorimeter will be on the lab bench and filled with 200 mL water. Make certain thestirrer is On (you should be able to see the shaft rotating). In the thermometer window clickSave to begin recording data. Allow 20-30 seconds to obtain a baseline temperature of thewater.4. Drag the weigh paper with the sample to the calorimeter until it snaps into place and thenthe sample into the calorimeter. Observe the change in temperature until it reaches amaximum and then record data for an additional 20-30 seconds. Click Stop. (You can click onthe clock on the wall labeled Accelerate to accelerate the time in the laboratory.) A data linkicon will appear in the lab book. Click the data link icon and record the initial and final watertemperatures in the data table. If you need to repeat this part of the experiment, enter theStockroom and select the preset experiment called Heat of Solution-NaOH on the clipboard.pourReaction 25. Click the red disposal bucket to clear the lab. Click on the Stockroom to enter. Click on theclipboard and select the preset experiment called Heat of Reaction: HCl(ag) + NaOH(s).Return to the laboratory.6. There will be a bottle of NaOH near the balance. A weigh paper will be on the balance withapproximately 4 g NaOH on the paper. Record the mass of NaOH in the data table. Thecalorimeter will be on the lab bench filled with 100 mL water, and there will be a beakercontaining 100 mL of 1.000 M HCl on the lab bench. In the thermometer window click Saveto begin recording data. Allow 20-30 seconds to obtain a baseline temperature of the water.7. Make sure the beaker of HCl is visible and drag it to the calorimeter and pour it into thecalorimeter. The HCl and the water are at the same temperature so there should be notemperature change. Now drag the weigh paper with the NaOH to the calorimeter until itsnaps into place and pour the sample into the calorimeter. It is important that the HCl beadded first and the NaOH added second. Observe the change in temperature until it reaches amaximum and then record data for an additional 20-30 seconds. Record the temperaturebefore adding the HCl and the temperature after adding the NaOH in the data table.Reaction 3In the thermometer window click Save to begin recording data. Allow 20-30 seconds to obtain abaseline temperature of the water. Pour the left beaker containing 100 mL of 1.0000M HCl intothe empty calorimeter and then pour the right beaker containing 100 mL of 1.0000M NAOH into Data TableParameterReaction 1 Reaction 2 Reaction 3Mass NaOH3.99834.0013initial temperature (° C)252525final temperature (° C)30.2135.0731.07

a) 100ml + 100ml = 200ml x 1.0g/ml = 200 gramsb) heat = mass x specific heat x delta temperature=…

Answered: Calculate the mass of the reaction…

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...