AP Chemistry
6.6 Introduction to Enthalpy of Reaction
6.4 Heat Capacity and Calorimetry
A student performs a calorimetry experiment to determine the molar enthalpy of neutralization, \(\Delta H_{\text{neutralization}}\), for the reaction represented below:
\[\text{HCl}(aq) + \text{NaOH}(aq) \rightarrow \text{NaCl}(aq) + \text{H}_2\text{O}(l)\]
The student mixes \(50.0\text{ mL}\) of \(1.00\text{ M HCl}(aq)\) and \(50.0\text{ mL}\) of \(1.00\text{ M NaOH}(aq)\), both initially at \(22.0\text{ }^\circ\text{C}\), in a polystyrene cup calorimeter. During the trial, the lid of the calorimeter is left off, allowing a significant amount of thermal energy to escape to the surrounding room before the maximum temperature is recorded. Which of the following best explains how this error affects the calculated magnitude of \(\Delta H_{\text{neutralization}}\)?
\[\text{HCl}(aq) + \text{NaOH}(aq) \rightarrow \text{NaCl}(aq) + \text{H}_2\text{O}(l)\]
The student mixes \(50.0\text{ mL}\) of \(1.00\text{ M HCl}(aq)\) and \(50.0\text{ mL}\) of \(1.00\text{ M NaOH}(aq)\), both initially at \(22.0\text{ }^\circ\text{C}\), in a polystyrene cup calorimeter. During the trial, the lid of the calorimeter is left off, allowing a significant amount of thermal energy to escape to the surrounding room before the maximum temperature is recorded. Which of the following best explains how this error affects the calculated magnitude of \(\Delta H_{\text{neutralization}}\)?
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