How much heat is produced when 100 mL of 0.250 M HCl...

How much heat is produced when 100 mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M $\mathrm{NaOH}$ (density, 1.00 g/mL) are mixed? $$\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H^{\circ}=-58 \mathrm{kJ}$$ If both solutions are at the same temperature and the heat capacity of the products is $4.19 \mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}$, how much will the temperature increase? What assumption did you make in your calculation?

How much heat is produced when 100 mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M $\mathrm{NaOH}$ (density, 1.00 g/mL) are mixed?
$$\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H^{\circ}=-58 \mathrm{kJ}$$
If both solutions are at the same temperature and the heat capacity of the products is $4.19 \mathrm{J} / \mathrm{g}^{\circ} \mathrm{C}$, how much will the temperature increase? What assumption did you make in your calculation?

Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It allows one to determine the amounts of substances consumed and produced, which is essential in calculating the energy change associated with the reaction.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed during a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reagent is necessary to accurately calculate the heat released or absorbed in the reaction.

Enthalpy Change of Reaction

The enthalpy change, often represented by ?H, is a measure of the heat absorbed or released during a chemical reaction at constant pressure. It is typically expressed in kilojoules per mole and is fundamental in energy balance calculations.

Calorimetry

Calorimetry is the experimental technique used to measure the amount of heat transferred in chemical or physical processes. It is based on the conservation of energy principle, where the heat produced by a reaction is assumed to be absorbed by the solution or calorimeter.

Specific Heat Capacity

Specific heat capacity is the amount of energy required to raise the temperature of a unit mass of a substance by one degree Celsius. It is a critical parameter for determining temperature changes in a system when heat is added or removed.

Assumption of No Heat Loss

In calorimetric calculations, it is commonly assumed that there is no heat loss to the surroundings. This assumption simplifies the analysis by allowing all the heat generated or absorbed in the reaction to be considered as entirely contributing to the temperature change of the system.

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