Question

Please help fill in data table and answer questions below table. thank you!

It was only 2 reactions, there is not a 4th. Please help with information provided.

DATA 1. Volume of 1.00 M HCI 2. Final temperature, t, 3. Initial temperature, t, 4. Change in temperature, t 5. Mass of solid 6. Heat, Reaction 2 (Mg) Reaction 1 (Mgo) 50.0 41.3 500 ml mL oC oC oC oC Mg kJ kJ 7. ΔΗ kJ kJ 8. Moles mol Mg mol MgO 9. ΔΗ/mo! kJ/mol kJ/mol 10. Determine ΔΗ/mol Mg for reaction (4). (10.) 11. Percent error Each student in the group must save their own copy of the experiment file tal you successfully saved your file, remove your flash drive. Outside of lab, you must print 2 individual graphs of temperature vs. time. One t Reaction 1 and one for Reaction 2. Open your LabQuest experiment file with Logger Double click anywhere in the graph window. Select the Axes Option tab. To displaya particular run, check it and uncheck the other. Click Done. From the Insert menu, Text Annotation and label each curve (Reaction 1 or Reaction 2) Each graph must also h or Pro select the Statisties box on it. PROCESSING THE DATA All calculations must be done in your lab notebook, submit the copy page(s) with your lab report. 1. Calculate the change in temperature,t- 2. Calculate the heat released by each reaction, q, using the formula , for Reactions I and 2 q Cp.m.t Cp 4.184 J/g C, and m 50.0 g of HCI solution. Convert joules to kJ in your final ansu 3, Determine ΔΗ. (ΔΗ--q) 4. Determine the moles of MgO and Mg used. 5. Use your Step 3 and Step 4 results to calculate AH/mol for MgO and Mg. 6. Determine AH mol Mg for Reaction 4. (Use your Step 5 results, your pre-lab work, and ΔΗ--285.8 kJ/mol for Reaction 3). 7. Determine the percent error for the answer you obtained in Step 6. Reaction 4 is the "formation reaction" for MgO. The accepted value for the enthalpy of formation for this reaction can be found in your general chemistry textbook. ed value-experimentalvalue1 x 100 00 error- accepted value This equation can be obtained by combining, in some way by equations (1), (2), and (3) ) Mgos) + 2 HCl(ag) MgCl2taHO) 2) Mg(s)2 HCla)MgCl2(aq) H2(e) (3) H2(g) 1/2 020)) The pre-lab exercise below requires you to combine equations (1), (2), and (3) to obtain equation (4) before you do the experiment. Do this and include it as a part of your experiment summary. Heats of reaction (AH) for equations (1) and (2) will be determined in this experiment. AH for reaction (3) is-285.8 kJ/mol of H0. PRE-LAB EXERCISE In the space provided below, combine equations (1). (2), and (3) to obtain equation (4) Mg0s) t 2 HCI(g) Mach (a)+H200 PROCEDIIRE

Answer 1

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