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PART 1: DATA [2 POINTS] Units: Molarity of HCl= Total: Apply Hess's Law to the experimental values of H1 and MH2 and the ilterature value for une standard formation of liquid water, AH3, to calculate the enthalpy of the combustion of magnesium, Hcombl(Mg). [1.5 points] 7. Galculate your % experimental error. [1 point] Accuracy: (grading use only) / [1 point] 8. Explain why your graphs of temperature versus time exhibit an increase in temperature. Also explain why the temperature reaches a maximum and then steadily decreases. [2 points] 9. The experimental procedure states that 1.5g of magnesium oxide are required. Will the calculated value for the enthalpy of reaction, H2, (Question 5) be affected if you used 1 of magnesium oxide instead? Explain why or why not. [2 points] 10. Explain why the reaction is performed inside a foam cup rather than in the usual glass beaker. How would your T and calculated H1 or H2 be affected if the reaction was performed in a beaker? [2 points] PART 1: DATA [2 POINTS] Units: Molarity of HCl= Total: Apply Hess's Law to the experimental values of H1 and MH2 and the ilterature value for une standard formation of liquid water, AH3, to calculate the enthalpy of the combustion of magnesium, Hcombl(Mg). [1.5 points] 7. Galculate your % experimental error. [1 point] Accuracy: (grading use only) / [1 point] 8. Explain why your graphs of temperature versus time exhibit an increase in temperature. Also explain why the temperature reaches a maximum and then steadily decreases. [2 points] 9. The experimental procedure states that 1.5g of magnesium oxide are required. Will the calculated value for the enthalpy of reaction, H2, (Question 5) be affected if you used 1 of magnesium oxide instead? Explain why or why not. [2 points] 10. Explain why the reaction is performed inside a foam cup rather than in the usual glass beaker. How would your T and calculated H1 or H2 be affected if the reaction was performed in a beaker? [2 points]