Heat Capacity & Calorimetry (College Board AP Chemistry)

A student investigates the enthalpy of solution, ΔH_soln, for two alkali metal halides, LiCl and NaCl. In addition to the salts, the student has access to a calorimeter, a balance with a precision of ±0.1 g, and a thermometer with a precision of ±0.1°C.

To measure ΔH_soln  for LiCl, the student adds 100.0 g of water initially at 15.0°C to a calorimeter and adds 10.0 g of LiCl(s) , stirring to After the LiCl dissolves completely, the maximum temperature reached by the solution is 35.6°C.

To explain why  ΔH_soln  for NaCl  is different than that for LiCl, the student investigates factors that affect ΔH_soln  and finds that ionic radius and lattice enthalpy (which can be defined as the ΔH associated with the separation of a solid crystal into gaseous ions) contribute to the process . The student consults references and collects the data shown in the table below.

Write the complete electron configuration for the Na⁺ ion in the ground

Using principles of atomic structure, explain why the Na⁺ ion is larger than the Li⁺ ion .

Which salt, LiCl or NaCl, has the greater lattice enthalpy? Justify your answer.

Below is a representation of a portion of a crystal of LiCl. Identify the ions in the representation by writing the appropriate formulas ( Li⁺ or Cl⁻ ) in the boxes below.

The lattice enthalpy of LiCl is positive, indicating that it takes energy to break the ions apart in LiCl. However, the dissolution of LiCl in water is an exothermic process. Identify all particle-particle interactions that contribute significantly to the dissolution process being exothermic. For each interaction , include the particles that interact and the specific type of intermolecular force between those particles.

2 C₃H₇OH(l) + 9O₂(g)  →  6CO₂(g) + 8H₂O(g)

A student performs an experiment to determine the enthalpy of combustion of 2-propanol, C₃H₇OH(l) , which combusts in oxygen according to the equation above. The student heats a sample of water by burning some of the C₃H₇OH(l) that is in an alcohol burner, as represented below. The alcohol burner uses a wick to draw liquid up into the flame. The mass of C₃H₇OH(l) combusted is determined by weighing the alcohol burner before and after combustion.

Data from the experiment are given in the table below.

Calculate the magnitude of the heat energy, in kJ, absorbed by the (Assume that the energy released from the combustion is completely transferred to the water.)

Based on the experimental data, if one mole of C₃H₇OH(l) is combusted, how much heat, in kJ, is released ? Report your answer with the correct number of significant

A second student performs the experiment using the same mass of water at the same initial temperature.

However, the student uses an alcohol burner containing  C₃H₇OH(l) that is contaminated  with water, which is miscible with C₃H₇OH(l) . The difference in mass of the alcohol burner before and after the combustion in this experiment is also 0.55 g. Would the final temperature of the water in the beaker heated by the alcohol burner in this experiment be greater than, less than, or equal to the final temperature of the water in the beaker in the first student's experiment? Justify your answer.

Na₂S₂O₃(aq) + 4 NaOCl(aq) + 2 NaOH(aq) → 2 Na₂SO₄(aq) + 4 NaCl(aq) + H₂O(l)

A student performs an experiment to determine the value of the enthalpy change, ΔH°_rxn, for the oxidation-reduction reaction represented by the balanced equation above.

Determine the oxidation number of Cl in NaOCl .

Calculate the number of grams of Na₂S₂O₃ needed to prepare 100.00 mL of 0.500 M Na₂S₂O₃(aq).

In the experiment, the student uses the solutions shown in the table below.

Using the balanced equation for the oxidation-reduction reaction and the information in the table above, determine which reactant is the limiting reactant. Justify your answer.

The solutions, all originally at 20.0°C, are combined in an insulated calorimeter. The temperature of the reaction mixture is monitored, as shown in the graph below.

According to the graph, what is the temperature change of the reaction mixture?

The mass of the reaction mixture inside the calorimeter is 15.21 g.

The student repeats the experiment, but this time doubling the volume of each of the reactants, as shown in the table below.

The magnitude of the enthalpy change, ΔH°_rxn, in kJ/mol_rxn, calculated from the results of the second experiment is the same as the result calculated in part (e)(ii) . Explain this result.

Write the balanced net ionic equation for the given reaction.

4 Fe(s) + 3 O₂( g) → 2 Fe₂O₃(s)      ∆H ° = − 1650 kJ / mol_rxn

A student investigates a reaction used in hand warmers, represented above. The student mixes Fe(s) with a catalyst and sand in a small open container. The student measures the temperature of the mixture as the reaction proceeds. The data are given in the following table.

The mixture (Fe(s), catalyst, and sand) has a total mass of 15.0 g and a specific heat capacity of 0.72  J/(g·°C). Calculate the amount of heat absorbed by the mixture from 0 minutes to 4 minutes.

Calculate the mass of Fe(s), in grams, that reacted to generate the amount of heat calculated in part (a).

In a second experiment, the student uses twice the mass of iron as that calculated in part (b) but the same mass of sand as in the first experiment. Would the maximum temperature reached in the second experiment be greater than, less than, or equal to the maximum temperature in the first experiment? Justify your answer.