Calculate the energy change for the reaction NH4Cl(s) ⟶NH3(g)+HCl(g) from the following: (

step 1 To determine the standard delta G for the following reaction, given three reactions, we need to

Calculate the energy change for the reaction NH4Cl(s)...

Calculate the energy change for the reaction $$ \begin{array}{ll} \mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \text { from the following: (9.6) } \\ \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g) & \Delta H=-184 \mathrm{~kJ} \\ \mathrm{~N}_{2}(g)+4 \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NH}_{4} \mathrm{Cl}(s) & \Delta H=-631 \mathrm{~kJ} \\ \mathrm{~N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) & \Delta H=-296 \mathrm{~kJ} \end{array} $$

Calculate the energy change for the reaction
$$
\begin{array}{ll}
\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \text { from the following: (9.6) } \\
\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g) & \Delta H=-184 \mathrm{~kJ} \\
\mathrm{~N}_{2}(g)+4 \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NH}_{4} \mathrm{Cl}(s) & \Delta H=-631 \mathrm{~kJ} \\
\mathrm{~N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) & \Delta H=-296 \mathrm{~kJ}
\end{array}
$$

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Key Concepts

Thermochemical Equations

These equations include both the chemical reaction and the corresponding enthalpy change, indicating whether the process is endothermic or exothermic. They provide a precise method of accounting for energy changes in reactions, which is essential for understanding reaction energetics.

Reaction Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It is critical for balancing chemical equations and ensures that the enthalpy changes are appropriately scaled with the number of moles of substances involved.

Hess's Law

This law states that the total enthalpy change for a reaction is the same regardless of the pathway taken. It allows the calculation of an unknown reaction's enthalpy change by combining and manipulating other reactions with known enthalpies, making it a fundamental tool in thermochemistry.

Enthalpy Change

Enthalpy change, often expressed in kilojoules (kJ), represents the heat absorbed or released during a chemical reaction at constant pressure. It is used to quantify the energy change associated with forming or breaking chemical bonds in a reaction.

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