Guide Questions for All Experiments
Guide Questions
Experiment 1
Calibration of the calorimeter:
1. Give the net ionic thermochemical equation of the reaction used to calibrate the calorimeter.
a. Is the reaction endothermic or exothermic?
b. Which is the limiting reactant?
c. How much (in moles) limiting reactant was used?
d. How much heat was generated (or absorbed) by the reaction?
2. Relate the sign of the ΔT to the ΔH of the reaction used for calibration.
3. What is the heat capacity of the calorimeter? Relate its sign to the sign of the ΔT.
4. In the appendix, show the derivation to obtain the equation used to calculate the heat capacity of the calorimeter.
Determination of Heats of Reaction:
5. Give the net ionic equation for each reaction.
6. Determine the limiting reactant and the amount of the limiting reactant in each of the reaction performed.
7. Calculate for the theoretical and experimental enthalpy of each reaction.
a. Determine whether the reaction is endothermic or exothermic.
b. Give the %error of your experimental values.
8. Relate the sign of ΔT to the sign of the experimental ΔH.
9. For reactions 1 – 4, which pair gave the most and the least exothermic (or endothermic) reaction? Explain the observation. (Use both the theoretical and experimental values to answer this)
10. For reactions 5 and 6, which gave the most exothermic reaction? Why? (Use both the theoretical and experimental values to answer this)
11. For reactions 7 and 8, what are the solid products of the reaction? What is the theoretical yield of each?
12. Reaction 8 is a synthesis (combination) reaction. Using the theoretical ΔH of the reaction, deduce the relative magnitude of the energy of bond breaking and bond formation during the reaction.
13. In the appendix, show the equation used to determine the heats of reaction for reactions 1 – 6 and reactions 7 and 8.
14. Tabulate the possible sources of errors and their effect to the following parameters: ΔT, Ccal and ΔH. Accompany
Experiment 1
Calibration of the calorimeter:
1. Give the net ionic thermochemical equation of the reaction used to calibrate the calorimeter.
a. Is the reaction endothermic or exothermic?
b. Which is the limiting reactant?
c. How much (in moles) limiting reactant was used?
d. How much heat was generated (or absorbed) by the reaction?
2. Relate the sign of the ΔT to the ΔH of the reaction used for calibration.
3. What is the heat capacity of the calorimeter? Relate its sign to the sign of the ΔT.
4. In the appendix, show the derivation to obtain the equation used to calculate the heat capacity of the calorimeter.
Determination of Heats of Reaction:
5. Give the net ionic equation for each reaction.
6. Determine the limiting reactant and the amount of the limiting reactant in each of the reaction performed.
7. Calculate for the theoretical and experimental enthalpy of each reaction.
a. Determine whether the reaction is endothermic or exothermic.
b. Give the %error of your experimental values.
8. Relate the sign of ΔT to the sign of the experimental ΔH.
9. For reactions 1 – 4, which pair gave the most and the least exothermic (or endothermic) reaction? Explain the observation. (Use both the theoretical and experimental values to answer this)
10. For reactions 5 and 6, which gave the most exothermic reaction? Why? (Use both the theoretical and experimental values to answer this)
11. For reactions 7 and 8, what are the solid products of the reaction? What is the theoretical yield of each?
12. Reaction 8 is a synthesis (combination) reaction. Using the theoretical ΔH of the reaction, deduce the relative magnitude of the energy of bond breaking and bond formation during the reaction.
13. In the appendix, show the equation used to determine the heats of reaction for reactions 1 – 6 and reactions 7 and 8.
14. Tabulate the possible sources of errors and their effect to the following parameters: ΔT, Ccal and ΔH. Accompany