DATA AND CALCULATIONS 1. Volume of 1.00 M HCI 2. Final temperature, 3. Initial temperature, f 4. Change in temperature,

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Data And Calculations 1 Volume Of 1 00 M Hci 2 Final Temperature 3 Initial Temperature F 4 Change In Temperature 1 (46.91 KiB) Viewed 36 times

Data And Calculations 1 Volume Of 1 00 M Hci 2 Final Temperature 3 Initial Temperature F 4 Change In Temperature 2 (64.21 KiB) Viewed 36 times

DATA AND CALCULATIONS 1. Volume of 1.00 M HCI 2. Final temperature, 3. Initial temperature, f 4. Change in temperature, at 5. Mass of solid 6. Heat, q 7. AH 8. Moles 9. AH/mol 11. Percent error Reaction 1 (MgO) 100 34.71 10. Determine AH'mol Mg for reaction (4)". (1) (2) (3) 8.7 9 "C 'C 'C 9 kj kJ mol MgO kJ/mol Reaction 2 (Mg) (60) 47-93 25-70 0-509 9 'C 'C 'C 9 kJ mol Mg kJ/mol kJ/mol
Heat of Combustion: Magnesium Reaction 2 9. Repeat Steps 3-8 using about 0.50 g of magnesium ribbon rather than magnesium oxide powder. The magnesium ribbon has been pre-cut to the proper length by your teacher. Be Pure to record the measured mass of the magnesium. CAUTION: Do not breathe the vapors produced in the reaction! PROCESSING THE DATA 1. In the spaces provided, calculate the change in temperature, Ar, for Reactions 1 and 2. 2. Calculate the heat released by each reaction, q, using the formula q=Cp-m-St Cp=4.18 J/g°C, and m= 100.0 g of HCl solution. Convert joules to kJ in your 3. Determine AH. (AH = -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 AH=-285.8 kJ for Reaction 3). final answer. 7. Determine the percent error for the answer you obtained in Step 6. The accepted value for this reaction can be found in a table of standard heats of formation.