Filling in the following table with the data obtained from the virtual calorimetry simulation. Calorimetry SimulationReaction 1Reaction 2Reaction 3 Mass of Water (g)N/A N/A Mass of NaOH Solid (g)N/A Molarity of NaOH Solution (mol/L)N/A N/A Volume of NaOH Solution (mL)N/A N/A Molarity of HCl Solution (mol/L)N/A Volume of HCl Solution (mL)N/A Initial Temperature (Tinitial,°C)Highest Temperature Reached (Tfinal,°C)Note: Assume the density of any solvent/solution mentioned in the table above is 1.00 g/mL and that the specific heat capacity of any resultant solution from Reactions 1, 2 and 3 is 4.184 J/(g·°C)Complete the Calculations and Results Section with these assumptions in your mind.
3 Calculations and Results:Filling in the following tables. In the empty space in the table, make sure to show complete calculations (show general equations and plug in your values) for each reaction and reporting your results with proper sig. figs. and units in the result column on the right. Reaction 1 CalculationsResultsMass of Solution Mass of SolutionΔT qsoln = Moles of NaOH = ΔHreaction1 = Reaction 2 CalculationsResultsMass of Solution ΔT qsoln = Moles of NaOH = ΔHreaction2 =
4 Reaction 3 CalculationsResultsMass of Solution ΔT qsoln = Moles of NaOH Moles of NaOH ΔHreaction3 = Questions: 1. Show that the two equations for reactions 1 and 3 shown below can be added algebraically to give the equation for reaction 2 in the middle. NaOH(s) Na+(aq) + OH- (aq) Reaction 1 NaOH(s) + H+(aq) + Cl- (aq) H2O(l) + Na+(aq) + Cl- (aq) Reaction 2 Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) H2O(l) + Na+(aq) + Cl-(aq) Reaction 3
5 2. Applying Hess’s Law and the result from the previous question, calculate the theoretical ΔH for reaction 2 using only the experimental ΔH values for reactions 1 and 3. NaOH(s) Na+(aq) + OH- (aq) ΔHreaction1 NaOH(s) + H+(aq) + Cl- (aq) H2O(l) + Na+(aq) + Cl- (aq) ΔHreaction2 Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) H2O(l) + Na+(aq) + Cl-(aq) ΔHreaction33. Compare the theoretically calculated enthalpy of reaction, ΔHtheoretical, for reaction 2 (from the previous question) with the experimentally determined enthalpy of reaction, ΔHexperimental, for reaction 2 (from simulation). Calculate the absolute difference between ΔHtheoretical and ΔHexperimental. Show your calculations. 4. If the absolute difference between ΔHtheoretical and ΔHexperimental is equal or less than 10 kJ/mol, then assume that the difference is negligible and that ΔHtheoretical = ΔHexperimental. According to your virtual experimental results, is Hess’s Law valid? Explain.
6 5. In reaction 1, a student measured the temperature of the resultant solution when some NaOH pellets were still left in the calorimeter. How does it affect the value of ΔHreaction1 ?
6. In reaction 2, a student forgot to put the lid back on the calorimeter after mixing NaOH pellet with HCl solution. How does it affect the value of ΔHreaction2 ?
7. In reaction 3, a student left the solution stirring for 30 min while talking to a friend. How does it affect the value of ΔHreaction3 ?
8. In this experiment, we assumed the density of water or any solution is 1.00 g/mL and that the specific heat capacity of any solution is 4.184 J/(g·°C) to simplify the calculation. List another assumption we made in this experiment.
