For the reactions H2( g)+Cl2( g) ⟶2 HCl(g)+X1 kJ 2 IICl(g) ⟶1 I2( g)+Cl2( g) X2 kJ (1) X1 an

step 1 For the reaction given as you can see on the screen, the options are x1 and x2 are numerically e

For the reactions H2( g)+Cl2( g) ⟶2 HCl(g)+X1 kJ 2 IICl(g)...

For the reactions $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{HCl}(\mathrm{g})+X_{1} \mathrm{~kJ}$ $2 \mathrm{IICl}(\mathrm{g}) \longrightarrow 1 \mathrm{I}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \quad X_{2} \mathrm{~kJ}$ (1) $X_{1}$ and $X_{2}$ are numerically cqual. (2) $X_{1}$ and $X_{2}$ are numerically different. (3) $X_{1} \quad X_{2}>\mathrm{O}$ (4) $X_{1} \quad X_{2}<0$

For the reactions $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{HCl}(\mathrm{g})+X_{1} \mathrm{~kJ}$
$2 \mathrm{IICl}(\mathrm{g}) \longrightarrow 1 \mathrm{I}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \quad X_{2} \mathrm{~kJ}$
(1) $X_{1}$ and $X_{2}$ are numerically cqual.
(2) $X_{1}$ and $X_{2}$ are numerically different.
(3) $X_{1} \quad X_{2}>\mathrm{O}$
(4) $X_{1} \quad X_{2}<0$

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Key Concepts

Thermochemical Equations

Thermochemical equations include both the chemical species and the energy change associated with the reaction, typically expressed in kilojoules (kJ). They provide a snapshot of the overall energy balance in a reaction by showing the energy absorbed or released, which helps in understanding the thermodynamic nature of the process.

Enthalpy Change and Sign Conventions

The enthalpy change (?H) of a reaction indicates whether a reaction is exothermic or endothermic. When energy is released during a reaction, it is properly represented as being on the product side of the equation, and the ?H is negative even if the numerical value given (such as kJ) is positive. Conversely, if energy is absorbed, the energy term appears on the reactant side and ?H is positive. This convention is crucial for correctly interpreting thermochemical data.

Exothermic vs Endothermic Reactions

Exothermic reactions release energy into the surroundings and are characterized by a negative enthalpy change even though the numerical value may be given as a positive number in a thermochemical equation. Endothermic reactions, on the other hand, require energy input and thus have a positive enthalpy change. Understanding these differences is essential when analyzing energy changes in chemical reactions.

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