Chapter 5: Problem 104
A quantity of \(85.0 \mathrm{~mL}\) of \(0.600 \mathrm{M} \mathrm{HCl}\) is mixed with \(85.0 \mathrm{~mL}\) of \(0.600 \mathrm{M} \mathrm{KOH}\) in a constant- pressure calorimeter. The initial temperature of both solutions is the same at \(17.35^{\circ} \mathrm{C}\), and the final temperature of the mixed solution is \(19.02^{\circ} \mathrm{C}\). What is the heat capacity of the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\).
Short Answer
Step by step solution
Calculate the Heat Absorbed by the Solution
Convert Heat from J to kJ
Calculate Moles of Water Produced
Calculate Heat Released by Neutralization
Determine Heat Capacity of the Calorimeter
Calculate the Heat Capacity of the Calorimeter
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Heat Capacity
The heat capacity can be expressed in different units, typically Joules per degree Celsius (J/°C) or kilojoules per degree Celsius (kJ/°C), and it is critical for accurately interpreting calorimetry experiments.
Neutralization Reaction
The balanced chemical equation is:\[\text{HCl}_{(aq)} + \text{KOH}_{(aq)} \rightarrow \text{KCl}_{(aq)} + \text{H}_2\text{O}_{(l)}\]During a neutralization reaction, an exothermic reaction typically occurs, releasing energy in the form of heat. This release is due to the formation of strong water bonds when hydrogen ions \((\text{H}^+)\) from the acid combine with hydroxide ions \((\text{OH}^-)\) from the base.
The heat released in neutralization reactions is characterized by the molar heat of neutralization, often measured in kJ/mol. In the given problem, it is \(-56.2 \text{ kJ/mol}\), indicating that the process is exothermic and releases 56.2 kJ of energy per mole of water formed.
Specific Heat Capacity
This assumption simplifies calculations by allowing us to apply the specific heat formula \[q = mc\Delta T\]where \( m \) is mass, \( c \) is specific heat capacity, and \( \Delta T \) is the change in temperature. Specific heat capacity is a critical factor in identifying how materials respond to heat changes, and it varies for different substances. Understanding it enables accurate prediction of temperature changes in reaction mixtures.
Enthalpy Change
- Endothermic reactions absorb heat (\( \Delta H > 0 \)).
- Exothermic reactions release heat (\( \Delta H < 0 \)).
Calculating enthalpy changes is essential in calorimetry as it allows chemists to understand energy dynamics in reactions. It provides insights into energy efficiency and the feasibility of industrial chemical processes.