In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed. Both so

step 1 Using the information in this question, let's calculate the empathy change for the neutralizatio

In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and...

In a coffee-cup calorimeter, 100.0 $\mathrm{mL}$ of 1.0 $\mathrm{M}$ NaOH and 100.0 $\mathrm{mL}$ of 1.0 $\mathrm{M} \mathrm{HCl}$ are mixed. Both solutions were originally at $24.6^{\circ} \mathrm{C}$ . After the reaction, the final temperature is $31.3^{\circ} \mathrm{C}$ . Assuming that all the solutions have a density of 1.0 $\mathrm{g} / \mathrm{cm}^{3}$ and a specific heat capacity of $4.18 \mathrm{J} / \mathrm{C} \cdot \mathrm{g},$ calculate the enthalpy change for the neutralization of $\mathrm{HCl}$ by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

Key Concepts

Calorimetry

Calorimetry is the branch of thermodynamics that focuses on measuring the amount of heat exchanged during physical and chemical processes. It involves using devices called calorimeters to quantify heat changes in reactions, phase transitions, or other processes, thereby providing insights into reaction energetics.

Constant Pressure Calorimetry

Constant pressure calorimetry refers to measuring heat changes under conditions where the pressure remains nearly constant, such as in a coffee-cup calorimeter. This context permits the direct determination of the enthalpy change (?H) of a reaction since at constant pressure, the heat exchanged is equal to the change in enthalpy.

Enthalpy Change

Enthalpy change (?H) is a thermodynamic quantity that represents the heat absorbed or released during a chemical reaction at constant pressure. It is a key measure in understanding reaction energetics, indicating whether a reaction is exothermic (releases heat) or endothermic (absorbs heat).

Specific Heat Capacity

Specific heat capacity is a property of a substance that indicates the amount of heat required to raise the temperature of one gram of that substance by one degree Celsius. This concept is critical in calorimetry as it allows for the calculation of the total heat involved in a process by relating temperature changes to energy changes.

Energy Conservation and Heat Transfer

The principle of energy conservation states that energy cannot be created or destroyed, only transferred. In the context of calorimetry, it implies that the heat lost or gained by the reaction must be equal to the heat gained or lost by the surroundings, enabling the calculation of the energy change of the response system.

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