DATA AND CALCULATIONS 1. Mass of 1.00 M HCI g 2. Final temperature, 12 3. Initial temperature, I, 4. Change in temperature, Al 5. Mass of solid Reaction 1 Reaction 2 (Mgo) (Mg) 100 109 g 30 5 "C 35.1 C 24.1 " 24.3 "C 6.3 C 0.993 g 0.271 9. = 1099 84.1995 - 100 x 184 x 10.8 Please us 19 kJ T 10.8 g 6. Heat, MSAT e- 26355 kJ KJ 7. AH of moles ku kJ 8. Moles 0.2718 Mr man 0.9938 40.3044 Smol 24.305kmal mol Mgo mol Mg 9. AH/mol kJ/mol kJ/mol 10. Determine AH/mol Mg for reaction (4) (1) (2) (3) (4)" 11. Percent error mordoxpedical Expected 100 Determine At for the process by subtracting tinitial from final, as shown. At = final - l'initial Given the specific heat capacity of the substance, a can be calculated. Then AH can be calculated by dividing a by the numbers of moles of limiting reactant. The unit for AH is kJ/mol. In this experiment you will collect temperature and time values for the following reactions: Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) (2) Mgo(s) + 2HCl(aq) MgCl2(aq) + H2O(0) (3) You will use the thermochemical equations for these two reactions along with the previously given equation for the hydrogen/oxygen reaction (1), to calculate the AH value for the combustion of magnesium: 2Mg(s) + O2(g) 2Mgo (s) (4) This calculation is done by applying Hess's Law, which states: When reactions are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. Often in applying Hess's law, we must manipulate the equations involved, multiplying with appropriate coefficients, reversing equations, or both. So we arrange the series of chemical equations such that, when added together all species will cancel except for the reactants and products that appear in the overall reaction