The oxidation of NH3(g) to NO(g) in the Ostwald process must...

The oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ to $\mathrm{NO}(\mathrm{g})$ in the Ostwald process must be very carefully controlled in terms of temperature, pressure, and contact time with the catalyst. This is because the oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ can yield any one of the products $\mathrm{N}_{2}(\mathrm{g}), \mathrm{N}_{2} \mathrm{O}(\mathrm{g}), \mathrm{NO}(\mathrm{g})$ and $\mathrm{NO}_{2}(\mathrm{g}),$ depending on conditions. Show that oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ to $\mathrm{N}_{2}(\mathrm{g})$ is the most exothermic of the four possible reactions.

The oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ to $\mathrm{NO}(\mathrm{g})$ in the Ostwald process must be very carefully controlled in terms of temperature, pressure, and contact time with the catalyst. This is because the oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ can yield any one of the products $\mathrm{N}_{2}(\mathrm{g}), \mathrm{N}_{2} \mathrm{O}(\mathrm{g}), \mathrm{NO}(\mathrm{g})$
and $\mathrm{NO}_{2}(\mathrm{g}),$ depending on conditions. Show that oxidation of $\mathrm{NH}_{3}(\mathrm{g})$ to $\mathrm{N}_{2}(\mathrm{g})$ is the most exothermic of the four possible reactions.

Key Concepts

Exothermic Reaction

An exothermic reaction is one that releases energy, typically in the form of heat, to the surroundings. In the context of oxidation reactions, comparing exothermicity helps determine which reaction pathway is energetically most favorable. The most exothermic reaction typically has a larger negative enthalpy change, indicating a greater release of energy.

Hess’s Law

Hess’s Law states that the total enthalpy change for a reaction is the same, regardless of the number of steps by which the reaction occurs. This principle allows for the calculation of reaction enthalpies by summing the standard enthalpies of formation of the products minus those of the reactants, making it a powerful tool in reaction thermodynamics.

Standard Enthalpy of Formation

This concept involves the enthalpy change when one mole of a compound is formed from its elements in their standard states. It is fundamental in calculating the overall energy change of a reaction because it provides a reference point for comparing the energy content of reactants and products in various chemical processes.

Reaction Enthalpy

Reaction enthalpy is the total heat absorbed or released during a chemical reaction at constant pressure. It is calculated using the standard enthalpies of formation of reactants and products. Understanding reaction enthalpy is crucial for determining the energy profile of a reaction and assessing its feasibility under given conditions.

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