Consider the reaction 2 HCl(a q)+Ba(OH)2(a q) ⟶BaCl2(a q)+2 H2 O(l) ΔH=-118 kJ Calculate the he

step 1 Hey guys, and this problem will calculate the final temperature of the mixture. Let's start. The

Consider the reaction 2 HCl(a q)+Ba(OH)2(a q) ⟶BaCl2(a q)+2...

Consider the reaction $2 \mathrm{HCl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow \mathrm{BaCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$ $\Delta H=-118 \mathrm{~kJ}$ Calculate the heat when $100.0 \mathrm{~mL}$ of $0.500 \mathrm{M} \mathrm{HCl}$ is mixed with $300.0 \mathrm{~mL}$ of $0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$. Assuming that the temperature of both solutions was initially $25.0^{\circ} \mathrm{C}$ and that the final mixture has a mass of $400.0 \mathrm{~g}$ and a specific heat capacity of $4.18 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}$, calculate the final temperature of the mixture.

Consider the reaction
$2 \mathrm{HCl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow \mathrm{BaCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$
$\Delta H=-118 \mathrm{~kJ}$
Calculate the heat when $100.0 \mathrm{~mL}$ of $0.500 \mathrm{M} \mathrm{HCl}$ is mixed
with $300.0 \mathrm{~mL}$ of $0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$. Assuming that the temperature of both solutions was initially $25.0^{\circ} \mathrm{C}$ and that the final mixture has a mass of $400.0 \mathrm{~g}$ and a specific heat capacity of $4.18 \mathrm{~J} /{ }^{\circ} \mathrm{C} \cdot \mathrm{g}$, calculate the final temperature of the mixture.

Key Concepts

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. This concept is essential for relating the heat energy absorbed or released by a system to the resulting temperature change, as expressed in the formula q = m × c × ?T.

Molarity

Molarity is a measure of concentration defined as the number of moles of a solute per liter of solution. It is used to quantify the amounts of reactants in solutions and establishes the basis for stoichiometric calculations in reactions conducted in the liquid phase.

Calorimetry

Calorimetry is the experimental technique used to measure the amount of heat exchanged in a physical or chemical process. It involves quantifying the thermal energy change of the system by monitoring temperature changes in a substance with known mass and specific heat capacity.

Limiting Reactant

The concept of a limiting reactant refers to the reactant that is completely consumed first in a chemical reaction, thereby determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for accurately predicting the extent of the reaction and the resulting energy changes.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the amounts of reactants and products in a reaction. It provides the mole ratios that dictate how much of each substance reacts or is produced, forming the foundation for calculations in reaction yield and heat changes.

Enthalpy Change

Enthalpy change (?H) is the amount of heat absorbed or released during a chemical reaction at constant pressure. It is an essential concept in thermochemistry, representing the energy transfer between the system and its surroundings, and indicates whether a reaction is exothermic or endothermic.

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