Answer Happy

Data Table Parameter Reaction 1 Reaction 2 Reaction 3 NA Mass of NaOH (6) 3.9983y 4.0013, Initial temperature (°C) 25.00°C 25.00°C 25.00°C Final temperature (°C) 30.21°C 35.07°( 31.07°C CALCULATIONS TABLE Total heat released Moles of NaOH (kJ) Rx'n # Mass of R'xn mixture (B) AT (C) Heat released per mol of NaOH (kJ/mol) 1 1 N 3

Conclusions: Complete the table below by writing a balanced net ionic equation for each part of this experiment with the corresponding enthalpy change (AH) Rxn Balanced Net Ionic Equation AH (kJ/mol) 1 N 3

Calculations: 1. Determine the change in temperature, At, for each reaction. Record your results in the results table in Step 15. 2. Calculate the mass of the reaction mixture in each reaction. (To do this, first determine the total volume of the solution. Then calculate the mass of the solution, based on the assumption that the added solid does not change the volume and that the density of the solution is the same as that of pure water, 1.00 g/mL.) Remember to add the mass of the solid to the mass of solution in Reactions 1 & 2. Record your results in the calculations table. 3. Calculate the total heat released in each reaction, in J, assuming that the specific heat capacity of the solution is the same as that of pure water, 4.184 /g"C. Record the result in the calculations table. (Remember: heat of reaction = mxC XAT) 4. Calculate the number of moles of NaOH used in reactions 1 and 2 where n = m/MW. Record the results in the calculations table. 5. Calculate the number of moles of NaOH used in reaction 3 by multiplying the volume of NaOH times the molarity (1.000 mol/L). Record the results in the calculations table. 6. Calculate the enthalpy change, in kJ/mol, of NaOH for each reaction and record the results in the calculations table. (Show calculations for each reaction in the spaces below or attach additional pages; Round answers to 3 sig figs) Reaction 1 @

Reaction 1 Reaction 2 Reaction 3