Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq)+NaC

step 1 Okay, so for this question, the first thing that we need to do is calculate the amount of energy

Insoluble AgCl(s) precipitates when solutions of AgNO3(aq)...

Insoluble AgCl(s) precipitates when solutions of $\mathrm{AgNO}_{3}(\mathrm{aq})$ and $\mathrm{NaCl}(\mathrm{aq})$ are mixed. $\operatorname{AgNO}_{3}(\mathrm{aq})+\mathrm{NaCl}(\mathrm{aq}) \rightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{NaNO}_{3}(\mathrm{aq})$ $$ \Delta_{i} H^{0}=? $$ To measure the energy evolved in this reaction, 250. mL. of 0.16 M AgNO $_{3}$ (aq) and 125 mL. of $0.32 \mathrm{M} \mathrm{NaCl}(\mathrm{aq})$ are mixed in a coffee-cup calorimeter. The temperature of the mixture rises from $21.15^{\circ} \mathrm{C}$ to $22.90^{\circ} \mathrm{C} .$ Calculate the enthalpy change for the precipitation of $\mathrm{AgCl}(\mathrm{s}),$ in $\mathrm{kJ} / \mathrm{mol}$. (Assume the density of the solution is $1.0 \mathrm{g} / \mathrm{mL}$ and its specific heat capacity is $4.2 \mathrm{J} / \mathrm{g} \cdot \mathrm{K} .)$

Insoluble AgCl(s) precipitates when solutions of $\mathrm{AgNO}_{3}(\mathrm{aq})$ and $\mathrm{NaCl}(\mathrm{aq})$ are mixed.
$\operatorname{AgNO}_{3}(\mathrm{aq})+\mathrm{NaCl}(\mathrm{aq}) \rightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{NaNO}_{3}(\mathrm{aq})$
$$
\Delta_{i} H^{0}=?
$$
To measure the energy evolved in this reaction,
250. mL. of 0.16 M AgNO $_{3}$ (aq) and 125 mL. of $0.32 \mathrm{M} \mathrm{NaCl}(\mathrm{aq})$ are mixed in a coffee-cup calorimeter. The temperature of the mixture rises from $21.15^{\circ} \mathrm{C}$ to $22.90^{\circ} \mathrm{C} .$ Calculate the enthalpy change for the precipitation of $\mathrm{AgCl}(\mathrm{s}),$ in $\mathrm{kJ} / \mathrm{mol}$. (Assume the density of the solution is $1.0 \mathrm{g} / \mathrm{mL}$ and its specific heat capacity is $4.2 \mathrm{J} / \mathrm{g} \cdot \mathrm{K} .)$

Key Concepts

Precipitation Reaction

A precipitation reaction occurs when two aqueous solutions react to form an insoluble solid, or precipitate. This concept involves understanding solubility rules and the formation of a solid product from ions in solution, which is crucial in predicting the outcome of mixing certain reactants.

Calorimetry

Calorimetry is the measurement of heat changes in chemical reactions using devices like a coffee-cup calorimeter. It involves recording temperature changes of the reaction mixture and converting these changes into energy values using the principles of heat capacity and mass, which are essential for determining the energetic profile of a reaction.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. It includes determining the number of moles of substances involved, identifying the limiting reagent, and establishing mole-to-mole conversions, which are fundamental for calculating yields and energy changes on a per mole basis.

Enthalpy Change

Enthalpy change is the heat absorbed or released during a chemical reaction at constant pressure. It represents the energy change associated with the bonds broken and formed during the reaction and is a key concept in thermodynamics, allowing comparison of energy profiles for different reactions on a standardized per mole basis.

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