In Part 1 of this experiment, you will measure the enthalpy change, H, for the reaction of magnesium metal with hydrochloric acid: Mg(s)+2H+(aq)Mg2+(aq)+H2(g)(Equation#11) The H for this reaction, H11, can be equated to: H11H11=Hf(products)Hf(reactants)={Hf[Mg2+(aq)]+Hf[H2(g)]}{Hf[Mg(s)]+2H[H+(aq)]}=Hf[Mg2+(aq)](eachoftheotherthreequantitiesisequaltozero) In other words, you have used your measurement of the enthalpy of a reaction to determine the standard enthalpy of formation of the magnesium ion, H[[Mg2+(aq)]. A student performed the first determination in Part 1. They reacted 59.74g of 1M HCl with 0.1945g of magnesium. The temperature before mixing was 18.4C and the temperature after mixing was 33.1C. 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 Answer: Your Answer Question 6 (1 point) A student performed the first determination in Part 1. They reacted 61.06g of 1M HCl with 0.1985g of magnesium. The temperature before mixing was 19.3C and the temperature after mixing was 33.5C. Calculate the heat flow (qrxn) based on this student's data. Report your final answer, in kJ, to 2 decimal places and only include the numerical value (no units). Do not use scientific notation to answer this question. Your