Looking for assistance with introduction, procedure and observation, please and thank you!

Hess's Law Lab Magnesium ribbon burns in air in a highly exothermic combustion reaction. A very bright flame accompanies the production of magnesium oxide, and therefore, it is impractical and dangerous to use a calorimeter to determine the enthalpy change for this reaction: (1) Mg(s)+21O2(g)MgO(s) Instead, you will determine the enthalpy changes for two other reactions (2), (3). You will use these enthalpy changes, along with the known enthalpy change for another reaction (4), to determine the enthalpy change for the combustion of magnesium. (2) MgO(s)+2HCl(aq)MgCl2(aq)+H2O(l) (3) Mg(s)+2HCl(aq)MgCl2(aq)+H2(g) (4) H2(g)+21O2(g)H2O(l)H=285.8kJ/mol Calculations: - Use the equation q=mcT to determine the amount of heat that is released by reactions (2) and (3). (only use the mass of HCl ) - Convert the mass of MgO and Mg to moles. Calculate H of each reaction in units of kJ/mol of MgO or Mg. Remember to put the proper sign in from of each H value. - Algebraically combine equation (2), (3), and (4), and their corresponding H values, to get equation (1) and H of the combustion of magnesium. - Based on the accepted value of H of the combustion of magnesium (601.6kJ/mol), calculate your percent error? Percentage Error =ActualValueExperimentalValueActualValue100 Analysis: - Compare the experimental value to the actual value. - State the percentage error and discuss reasons why two values may be different. - Identify the experimental errors that would be a part of this experiment. Name at least two and state their effects on the calculations. - Why is fair to assume that the HCl solution has the same density and specific heat capacity as water