Use the following data to work through problems 4-6.

• 50.0 mL of each solution was used in each experiment.
• Each solution had a molarity of 2.00 M.
• The density of the solutions once mixed are 1.03 g/mL.
• The following table is data collected from an actualexperiment.

	Initial Temp	Final Temp	Temp Change
NaOH + HCL	19.85	33.07	13.2
NaOH+ NH4Cl	19.78	20.40	0.62
HCl + NH3	20.16	32.05	11.89

1. Calculate the amount of heat energy,q_surroundings, produced in each reaction. Use03 g/mL for the density of all solutions. Use the specific heat ofwater, 4.184 J/(g•°C), for each of the three reactions.q_surroundings = C_s ´m ´ ∆T

1. Calculate the enthalpy change, ∆H_reaction,per mole of reactant for each of the three reactions in units ofkJ/mole.

                                   ∆H_reaction = ∆H_system

1. Calculate a percent error between the accepted values for∆H_reaction(use values calculated in question 1as accepted values) and the “experimental” values you calculated inquestion 5 for each reaction.

                                               

                       % Error = Experimental – Accepted x 100

                                               Accepted