In Part 2, you will measure the enthalpy change accompanying the reaction of magnesium oxide with hydrochloric acid. MgO(s)+2H+(aq)Mg2+(aq)+H2O(l)(Equation#12) H for this reaction, H12, is given by: H12=H[[Mg2+(aq)]+Hf[H2O(l)]H,[MgO(s)]2Hf[H+(aq)](Equation#13) In this reaction you obtain, by measurement, the value of H12. The value of H+[Mg2+(aq)] was found in Part 1 . H[H2O(l)] at 25C and 1atm is found in any table of standard enthalpies of formation, and is 285.8kJmol1 (any change in this value caused by a slightly different temperature and pressure in the laboratory will be considered negligible). Therefore, the enthalpy of formation of MgO(s),Hf[MgO(s)], may be calculated by rearranging equation (13). A student used 0.7217g of magnesium oxide in the first determination in Part 2. Calculate the number of moles of magnesium oxide this student would have used. Report your final answer, in moles, to 5 decimal places and only include the numerical value (no units). Do not use scientific notation to answer this question. Your Answer: Your Answer Question 11 (1 point) A student performed the first determination in Part 2. They reacted 61.56g of 1M HCl with 0.7093g of magnesium oxide. The temperature before mixing was 19.4C and the temperature after mixing was 29.5C. Calculate the heat capacity (Cp) of the final solution based on this student's data. Report your final answer, in J/K, to the nearest integer, and only include the numerical value (no units). Do not use scientific notation for this question. Your