Additivity of heats of reaction hess's law answer key

Hello, the following are two worksheets that need to be done, in order to get to answer them you will need to use BeyondLabz which I will help you access if you don't know how to.

FOR BEYOND LABZ HEAT OF REACTION: MGO (S) + HCL (AQ)
In this simulation you will use coffee cup calorimetry to measure the heat transfer that occurs when magnesium oxide reacts with hydrochloric acid. You will use your results to calculate the enthalpy of the reaction (LaTeX: \DeltaΔHrxn) and compare it to a predicted value calculated using values for standard enthalpy of formation.

FOR BEYOND LABZ HESS'S LAW
In this simulation you will use coffee cup calorimetry to measure the heat of reaction (LaTeX: \DeltaΔHrxn) for three reactions and show how they are related by Hess's Law. You have to record data for three different reactions.

Energy is either absorbed or released for all chemical reactions, and we call this energy the enthalpy of reaction (Hrxn). If the enthalpy of reaction is positive, then we say that the energy was absorbed or that the reaction was endothermic. If the enthalpy of reaction is negative, then we say that energy was released or that the reaction was exothermic. Most chemical reactions are exothermic. In this problem, you will measure the amount of heat released when solid MgO is reacted with aqueous HCl to form water and then you will calculate the heat of reaction. MgO(s) + 2 HCl(aq) ↔ H2O(l) + MgCl2(aq) 1. Start Virtual ChemLab, select Thermodynamics, and then select Heat of Reaction: MgO + HCl from the list of assignments. The lab will open in the Calorimetry laboratory. 2. There will be a bottle of MgO near the balance. A weigh paper will be on the balance with approximately 2.81 g MgO on the paper. Record the mass of MgO in the data table. 3. The empty calorimeter will be on the lab bench and there will also be a beaker filled with 100.0 mL of 1.000 M HCl. Drag the beaker to the calorimeter until it snaps into place and pour the HCl into the calorimeter. Make certain the stirrer is On (you should be able to see the shaft rotating). In the thermometer window click Save to begin recording data. Allow 20-30 seconds to obtain a baseline temperature of the HCl solution. Drag the weigh paper containing the MgO sample over to the calorimeter and drop the sample in. Observe the change in temperature until it reaches a maximum and then record data for an additional 20-30 seconds. Click Stop in the temperature window. (You can click on the clock on the wall labeled Accelerate to accelerate the time in the laboratory.) A data link icon will appear in the lab book. Click the data link icon and record the temperature before adding the MgO and the highest temperature after adding the MgO in the data table. (Remember that the water will begin to cool down after reaching the equilibrium temperature.) Data Table MgO/HCl Mass MgO (g) initial temperature (C) final temperature (C) 4. Is the observed reaction endothermic or exothermic? What will be the sign of Hrxn? 5. Calculate the change in temperature, T. Record your results in the table on the following page. 6. Calculate the mass of the reaction solution (MgO and HCl) in the calorimeter. (To do this, assume that the density of the HCl solution originally in the calorimeter can be approximated with the density of water (1.00 g/mL). Show your work here. Record your results in the results table. 7. Calculate the heat transfer for the reaction (qrxn), in J, assuming that the specific heat capacity of the solution is the same as that of pure water, 4.184 J/g.C. Show your work here. Record the result in the results table. 8. Calculate the number of moles of MgO used in the reaction. The molar mass of MgO is 40.304 g/mol. Show your work here. Record the results in the results table. 9. Calculate Hrxn, in kJ/mol, of MgO for the reaction and record the results in the results table. Make sure the sign of Hrxn is correct. Show your work here and record it in the results table.