Question

A student carries out the following reaction in lab by mixing 50.0 mL of a 1.00 M solution of hydrochloric acid with 50.0 mL of a 1.00 M solution of potassium hydroxide:

HCl (aq) + KOH (aq) --> KCl (aq) + H2O (l)
The average initial temperature of the two solutions was 25.00 °C. After mixing, the final temperature of the solution was 31.43 °C. The mass of the resulting solution was 100.2 g.

1. Determine the theoretical yield of KCl (in moles) of the student’s reaction.

2. Assuming that the specific heat capacity of the solutions that the student used are equal to the specific heat capacity of pure water, calculate the heat (qsolution) in kJ that was absorbed by the contents of the coffee cup from the reaction.

3. Calculate the value of ΔHrxn in the units kJ / mol KCl.

4. For this reaction, the theoretical value of ΔHrxn is –55.8 kJ / mol KCl. What was the student’s percent error when determining ΔHrxn?

Answer 1

Step-by-step explanation:

The amount of heat gained or lost by a sample (q) can be calculated using the equation q = mcΔT, where m is the mass of the sample, c is the specific heat, and ΔT is the temperature change.Apr 19, 2021

Answer 2

The student's theoretical yield of KCl is 0.0500 mol. The heat absorbed (q_solution) by the solution is 2.687 kJ. The student's calculated enthalpy change (ΔH_rxn) is 53.74 kJ/mol, which results in a percent error of 196.59% compared to the theoretical value of ΔH_rxn, which is -55.8 kJ/mol.

Step-by-step explanation:

1. The theoretical yield of KCl is determined by the stoichiometry of the reaction. Since both HCl and KOH are present in equal molar amounts, they will react in a 1:1 ratio according to the chemical equation HCl (aq) + KOH (aq) --> KCl (aq) + H2O (l). With 0.0500 mol of each reactant (calculated from the 50.0 mL of 1.00 M solutions), the theoretical yield of KCl is also 0.0500 mol.

2. To calculate the heat absorbed (qsolution) by the solution, use the formula q = m•c•ΔT, where m is the mass of the solution, c is the specific heat capacity (4.184 J/g°C for water), and ΔT is the change in temperature. Here, q = 100.2 g • 4.184 J/g°C • (31.43°C - 25.00°C) = 2686.892 J or 2.687 kJ.

3. To find the enthalpy change (ΔHrxn) per mole of KCl, divide the heat absorbed by the moles of KCl formed. ΔHrxn = 2.687 kJ / 0.0500 mol = 53.74 kJ/mol.

4. To calculate the percent error in the student's determination of ΔHrxn, use the formula: percent error = |(experimental value - theoretical value) / theoretical value| • 100%. Here, the percent error = |(53.74 kJ/mol)- (-55.8 kJ/mol)| / (-55.8 kJ/mol) • 100% = 196.59%.