A coffee-cup calorimeter contains 100.0 mL of 0.300 M HCl at...

A coffee-cup calorimeter contains $100.0 \mathrm{mL}$ of $0.300 \mathrm{M}$ HCl at $20.3^{\circ} \mathrm{C} .$ When $1.82 \mathrm{g} \mathrm{Zn}(\mathrm{s})$ is added, the temperature rises to $30.5^{\circ} \mathrm{C}$. What is the heat of reaction per mol Zn? Make the same assumptions as in Example $7-4,$ and also assume that there is no heat lost with the $\mathrm{H}_{2}(\mathrm{g})$ that escapes. $$\mathrm{Zn}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})$$

A coffee-cup calorimeter contains $100.0 \mathrm{mL}$ of $0.300 \mathrm{M}$ HCl at $20.3^{\circ} \mathrm{C} .$ When $1.82 \mathrm{g} \mathrm{Zn}(\mathrm{s})$ is added, the temperature rises to $30.5^{\circ} \mathrm{C}$. What is the heat of reaction per mol Zn? Make the same assumptions as in Example $7-4,$ and also assume that there is no heat lost with the $\mathrm{H}_{2}(\mathrm{g})$ that escapes.
$$\mathrm{Zn}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})$$

Key Concepts

Calorimetry

Calorimetry is the experimental process of measuring the amount of heat exchanged in a chemical reaction or physical change. It involves using a calorimeter, which is designed to either absorb or supply heat to determine the thermal energy change of the system.

Heat Capacity and Specific Heat

The heat capacity of a substance is the amount of heat required to change its temperature by a given amount, while specific heat is the heat required per unit mass per degree change in temperature. These concepts are essential for quantifying how much energy is absorbed or released when a substance, such as a solution, undergoes a change in temperature during a reaction.

Temperature Change

The observed change in temperature of the system is a crucial measurement in calorimetry. It reflects the net heat absorbed or released during a chemical reaction, which, when combined with the heat capacity or mass and specific heat of the system, allows for calculation of the energy change associated with the reaction.

Stoichiometry

Stoichiometry involves quantitative relationships between reactants and products in a chemical reaction. It is used to convert between masses and moles, ensuring that the calculated energy changes are expressed on a per mole basis, which is necessary for comparing the thermodynamic properties of different reactions.

Reaction Enthalpy

Reaction enthalpy, or the heat of reaction, is the energy change that occurs during a chemical reaction at constant pressure. Calculating the enthalpy change per mole of a reactant provides a standardized measure of the reaction's energetics, facilitating comparisons and further thermodynamic calculations.

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