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Unformatted text preview: Change in Temp- 14.1 degrees Celsius Part C: Mass of Power- 0.4 g Mass of Acid- 55.3g-3.91g= 51.39g Change in Temp- 2.0 degrees Celsius Part B &C: (Delta H*Molar Mass/Mass of Additive)*1 kJ/1000 J= delta H˚x Delta H˚1= -285.8 kJ/mol Delta H˚2= -573.283 kJ/mol Delta H˚3= -37.32 kJ/mol Due to the reactions, Reaction Heat of Magnesium: -324.803 J Conclusion The experiment was successful in determining the heat of reaction for the combustion of magnesium metal. However, a slight error did exist due to human error and faulty lab equipment. By using our understanding of Hess’ Law, we could rearrange the equations to find the value of the reaction to be -324.803 J. The negative sign indicates that the reaction is exothermic due to it giving off heat. Overall, the data provided a successful calculation of the heat from the magnesium combustion through Hess’ Law....
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