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

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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$M \mathrm{HCl}$ is mixed with 300.0 $\mathrm{mL}$ of 0.100$M \mathrm{Ba}(\mathrm{OH})_{2}$ . 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 $\mathrm{J} / \mathrm{C} \cdot \mathrm{g}$ , 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$M \mathrm{HCl}$ is mixed with 300.0 $\mathrm{mL}$ of 0.100$M \mathrm{Ba}(\mathrm{OH})_{2}$ . 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 $\mathrm{J} / \mathrm{C} \cdot \mathrm{g}$ , calculate the final temperature of the mixture.

Key Concepts

Specific Heat Capacity

Specific heat capacity is a property of a substance that indicates the amount of heat energy required to raise the temperature of one gram of the substance by one degree Celsius. In calorimetric calculations, it is used to relate the heat energy change to the observed temperature change of the reaction mixture.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation to understand the quantitative relationships between reactants and products. It allows you to determine how many moles of each substance are consumed or produced, which is essential for calculating the overall energy changes in a chemical reaction.

Limiting Reactant

The limiting reactant is 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 in both yield and energy calculations as it directly influences the extent of the reaction.

Enthalpy Change

Enthalpy change (?H) is the heat released or absorbed during a chemical reaction at constant pressure. This value, often provided per mole of reaction, indicates whether the reaction is exothermic (releases heat) or endothermic (absorbs heat), and is fundamental to understanding energy transfers during the reaction.

Calorimetry

Calorimetry is the technique used to measure the heat absorbed or released during a chemical reaction. It involves monitoring temperature changes in a system with a known mass and specific heat capacity, thereby allowing the calculation of energy changes associated with the reaction.

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