Question

please help fill in data table and answer questions. please show all work. thank you!

Reaction 2 (Ma Reaction 1 (Mgo) 1. Volume of 1.00 M HCT 2. Final temperature, t 3. Initial temperature, t, EO.O ml 50.0 mt 28 a0 oc 4. Change in temperature, t 5. Mass of solid 203 MgO 6. Heat, q k.J kJ kJ k.I 8. Moles mol Mg mol MgO 9. ΔΗ/mol kJ/mol kJ/mol 10. Determine ΔΗ/mol Mg for reaction (4). (10.) II. Percent error 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, ,, for Reactions 1 and 2 2. Calculate the heat released by each reaction, q, using the formula 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 answer. 3, Determine ΔΗ. (ΔΙ1--q) 4. Determine the moles of MgO and Mg used. · Use your Step 3 and Step 4 results to calculate ΔΗ/mol for MgO and Mg. Determine AH/mol Mg for Reaction 4. (Use your Step 5 results, your pre-lab work, and AH--285.8 kJ/mol for Reaction 3). 7. Determine the percent error for the answer you obtained in Step 6. Reaction 4 is the tion reaction" for MgO. The accepted value for the enthalpy of formation for this reaction can be found in your general chemistry textbook. % error = accepted value-experimental value x100 accepted value The pre-lab exercise below requires you to combine equations (I). (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. Δ11 for reaction (3) is-285.8 kJ/mol of H2O. PRE-LAB EXERCISE In the space provided below, combine equations (1). (2), and (3) to obtain equation (4)

Answer 1

-4 1843/gà = 29, Sc-208℃ = 1, 883KJ 4225 8 J A. 226 KJ H=一4.226 KJ Moles 2 1365 XIO 355x ID 412 29 K3

Cs) + 4,02(a) → OCS -285,8 MB897) K7ms) 4H = (-412, 29 @y Fmo": {-co-‘RT (-559. is) 2ne, laHİtng 10 4H 一601-7 7.077