Can you please help with reaction 2 and 3 under calculations? Lab - Heat of Reaction for the Combustion of MagnesiumAlthough you will not be working with actual chemicals during this laboratory, since you will bedoing it virtually, the procedure is given in order for you to be aware of the process that would befollowed in a laboratory setting.IntroductionIn this experiment, you will use Hess's Law to determine the heat for a reaction that is difficult tomeasure directly. Magnesium metal burns rapidly, releasing light and heat, as observed in photoflashbulbs or by burning magnesium ribbon. The reaction is presented by the equation:Mg(s) + 1/2O₂(g) →→→→→→MgO(s)This equation can be obtained by combining equations (2), (3) and (4):MgO(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂OMg(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂(g)H₂(g) + 1/2O2(g) → H₂O)Material(1)By combining these three equations, you can obtain equation (1). The heats of reaction forequations (2) and (3) can easily be determined by experiments. The heat of reaction forequation (4) can be obtained from a table of values for previously measured reactions.Procedure(2)REACTION 2:(3)Chemicalsmagnesium, magnesium oxide, hydrochloric acidApparatus:Polystyrene calorimeter, graduated cylinder, electronic balance, filter paper, spatula,thermometer, glass stirring rod, stop watch,(4)Safety• Safety goggles and a lab apron should always be worn when working with chemicals.This lab will be performed using small quantities of chemicals (micro-scale chemistry).REACTION 3:1. Pour 100 mL of 1.0 mol/L hydrochloric acid into your polystyrene calorimeter.2. Weigh out 1.00 g of magnesium oxide on a filter paper.3. Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁(precise to 0.1°C). It may take several seconds for the temperature to stabilize.Add the magnesium oxide powder to the solution.4.5. Use a glass stirring rod to stir the cup contents until a maximum temperature has beenreached and the temperature starts to drop.6. Record the maximum temperature, T₂1. Pour 100 mL of 1.0 M hydrochloric acid into your polystyrene calorimeter.2. Weigh out 0.50 g of magnesium ribbon (this is about 46 cm). Roll it up loosely around apencil so that you end up with a coil. Make sure it is not too tightly coiled.3. Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁(precise to 0.1°C). It may take several seconds for the temperature to stabilize.4. Add the magnesium ribbon to the solution.5. Use a glass stirring rod to stir the cup contents until maximum temperature has beenreached and the temperature starts to drop. This video shows a similar procedure. Watch the video and answer the questions belowa) What were 3 pieces of lab equipment you saw in the video?b) What were some of the safety precautions they mentioned?c) Were the reactions shown the same as the ones in this lab? How can you tell?ResultsUse the table of standard enthalpies of formation to calculate the theoretical value.Sample results are provided below.Table #1: Volume, Temperature and Mass Values for Reactions 2 and 3Volume of HCIFinal temperature (T₂)Initial temperature (T₁)Change in temperature (AT)Mass of solidCalculations:3. Convert your answer into kJ.4. How many moles of MgO were used?5. Convert your answer into kJ/mol MgO.Reaction 31. Combine equations (2), (3) and (4) to obtain equation (1).Reaction 2Reaction 2(MgO)32.1°C% error-24.0°CConclusion0.96 g#experimental - # actual# actual1. Calculate the change in temperature for reaction (2).2. Calculate the energy released (AH) in (2) (in J), using Q=mcAT. The mass to be used isthe mass of HCI. Assume the density of hydrochloric acid to be 1 g/mL.x 100Reaction 3(Mg)48.2°C1. Calculate the change in temperature for reaction (3).2. Calculate the energy released (AH) in (3) (in J), using Q=mcAT. The mass to be used isthe mass of HCI.24.0°C3. Convert your answer into kJ.4. How many moles of Mg were used?5. Convert your answer into kJ/mol Mg.6. Calculate the heat of reaction (1) in kJ/mol of MgO by combining (2), (3) and (4) andtheir AH values that you obtained, in order to get equation (1) and its AH for thecombustion of Mg.0.55 g7. Determine the theoretical value for the combustion of magnesium, from the table ofstandard enthalpies of formation.8. Calculate the percentage error.Briefly state the results for the laboratory, in general. This should be no more than twosentences.

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