Rewrite each equation below with the ΔH value included with either the reactants or the products

step 1 In each part of this problem, we are given a chemical reaction as well as a value for the change

Rewrite each equation below with the ΔH value included with...

Rewrite each equation below with the $\Delta H$ value included with either the reactants or the products, and identify the reaction as endothermic or exothermic. a. $\mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$ $\Delta H^{0}=-285.83 \mathrm{kJ}$ b. $2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s)$ $\Delta H^{0}=-1200 \mathrm{kJ}$ c. $\mathrm{I}_{2}(s) \longrightarrow \mathrm{I}_{2}(g) ; \Delta H^{0}=+62.4 \mathrm{kJ}$ d. $3 \mathrm{CO}(g)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)$$\Delta H^{0}=-24.7 \mathrm{kJ}$

Rewrite each equation below with the $\Delta H$ value included with either the reactants or the products, and identify the reaction as endothermic or exothermic.
a. $\mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$
$\Delta H^{0}=-285.83 \mathrm{kJ}$
b. $2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s)$
$\Delta H^{0}=-1200 \mathrm{kJ}$
c. $\mathrm{I}_{2}(s) \longrightarrow \mathrm{I}_{2}(g) ; \Delta H^{0}=+62.4 \mathrm{kJ}$
d. $3 \mathrm{CO}(g)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)$$\Delta H^{0}=-24.7 \mathrm{kJ}$

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Key Concepts

Thermochemical Equations

These are chemical equations that include the enthalpy change (?H) for the reaction, reflecting the overall energy change during the process. In these equations, energy can be shown as part of the reactants or products, which provides insight into whether energy is absorbed or released during the reaction.

Reaction Enthalpy (?H)

Reaction enthalpy is the heat change at constant pressure during a reaction. It is represented by ?H and can be either positive or negative. A negative ?H indicates that the reaction releases energy while a positive ?H indicates that the reaction absorbs energy, and it is directly related to the energy flow between the system and its surroundings.

Exothermic Reactions

Exothermic reactions release energy in the form of heat, which is why they have a negative ?H value. When writing thermochemical equations for exothermic reactions, the released energy is typically placed on the products side to emphasize that energy is a product of the reaction.

Endothermic Reactions

Endothermic reactions absorb energy from their surroundings, leading to a positive ?H value. In the notation of thermochemical equations, the absorbed energy is usually shown on the reactants side, indicating that additional energy is required for the reaction to proceed.

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