Write an equation for the formation of each compound from its elements in their standard states, and find ΔH °f for each in Appendix IIB. a. NH₃(g)

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Identify the elements in their standard states that make up ammonia (NH3). Nitrogen (N) is a diatomic gas (N2) and hydrogen (H) is a diatomic gas (H2) in their standard states.

Write the balanced chemical equation for the formation of ammonia from its elements. The balanced equation is: \( \frac{1}{2} N_2(g) + \frac{3}{2} H_2(g) \rightarrow NH_3(g) \).

Consult Appendix IIB of your textbook or another reliable source to find the standard enthalpy of formation (\( \Delta H^\circ_f \)) for ammonia (NH3).

Record the value of \( \Delta H^\circ_f \) for NH3. This value represents the change in enthalpy when 1 mole of ammonia is formed from nitrogen and hydrogen in their standard states under standard conditions.

Use the value of \( \Delta H^\circ_f \) for NH3 in any further calculations or discussions related to the thermodynamics or energetics of reactions involving ammonia.

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Standard State

The standard state of a substance refers to its physical state (solid, liquid, or gas) at a defined set of conditions, typically 1 bar of pressure and a specified temperature, usually 25°C. For elements, the standard state is the most stable form at these conditions. Understanding standard states is crucial for writing formation equations, as it ensures that the reactants are in their correct physical forms.

Formation Reaction

A formation reaction is a chemical reaction in which one mole of a compound is formed from its constituent elements in their standard states. The equation for the formation of a compound, such as NH3, must include the elements nitrogen and hydrogen in their standard states, which are N2(g) and H2(g), respectively. This concept is essential for accurately representing the synthesis of compounds.

Enthalpy of Formation (ΔH°f)

The enthalpy of formation (ΔH°f) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. It is a key thermodynamic quantity used to understand the energy changes associated with chemical reactions. Values for ΔH°f can be found in thermodynamic tables, and they are vital for calculating reaction enthalpies and understanding stability.

Write an equation for the formation of each compound from its elements in their standard states, and find ΔH °f for each in Appendix IIB. a. NH3(g)