Question

Standard enthalpies of formation are relative values. What are \(\Delta H_{\mathrm{f}}^{\circ}\) values relative to?

Short answer

The \(\Delta H_{\mathrm{f}}^{\circ}\) values are relative to the enthalpy of the constituent elements in their most stable forms (reference state) at standard conditions (1 atm and 298.15 K, or 25°C). For example, the reference state for hydrogen is H₂ gas, while for carbon, it is solid graphite.

Step-by-step solution

Defining standard enthalpy of formation

Standard enthalpy of formation, denoted by \(\Delta H_{\mathrm{f}}^{\circ}\), is the change in enthalpy during the formation of one mole of a substance at standard conditions (1 atm and 298.15 K, or 25°C) from its constituent elements in their most stable forms (reference state). It is an essential concept in thermodynamics to calculate the enthalpy changes in various chemical reactions.

Reference state of constituent elements

The \(\Delta H_{\mathrm{f}}^{\circ}\) values are relative to the enthalpy of the constituent elements in their most stable forms (reference state) at standard conditions. For example, the reference state for hydrogen is H2 gas, while for carbon it is solid graphite. Since these reference states are assigned an enthalpy value of zero, the standard enthalpy of formation measures the enthalpy change from these reference states to the formation of the compound. In conclusion, the \(\Delta H_{\mathrm{f}}^{\circ}\) values are relative to the enthalpy of the constituent elements in their most stable forms at standard conditions.

Key concepts

Thermodynamics

Thermodynamics is a fundamental branch of physics that deals with heat, work, and the transformation of energy. It plays a crucial role in understanding how substances interact and change, especially during chemical reactions.

One of the key concepts of thermodynamics is enthalpy (\(H\)), which is a measure of total heat content of a system. While energy can neither be created nor destroyed, it can change forms, and in chemical processes, enthalpy helps us track these energy transformations. Enthalpy changes can tell us how much heat is absorbed or released during a reaction, which is vital for predicting reaction behavior and determining reaction feasibility.

Enthalpy Change

Enthalpy change, denoted by \(\Delta H\), refers to the difference in enthalpy between the products and reactants during a chemical reaction. It's a crucial indicator used to determine whether a reaction is exothermic or endothermic.

For instance, when \(\Delta H\ < 0\), the reaction is exothermic, meaning it releases heat to the surroundings. Conversely, if \(\Delta H\ > 0\), the reaction absorbs heat, making it endothermic. The standard enthalpy of formation, \(\Delta H_{\mathrm{f}}^{\circ}\), is a specific type of enthalpy change that occurs when one mole of a compound forms from its elements in their standard states.

Chemical Reactions

Chemical reactions are processes in which substances, called reactants, transform into different substances, known as products. Each reaction comes with an associated enthalpy change that determines how energy is exchanged within the system.

In a reaction, the breaking of bonds within reactants (which requires energy) and the formation of new bonds in products (which releases energy) contribute to the overall enthalpy change. By using the standard enthalpies of formation for each compound involved, we can calculate the total enthalpy change for any given chemical reaction.

Reference State

The reference state is a predefined standard condition used as a basis for comparison in thermodynamics. For substances involved in chemical reactions, the reference state is often the most stable physical form of the element at 1 atmosphere of pressure and a temperature of 298.15 K (25°C).

When discussing enthalpy changes, particularly \(\Delta H_{\mathrm{f}}^{\circ}\), this concept ensures that all calculations start from a common ground. Assigning a value of zero enthalpy to elements in their reference state simplifies the calculation of enthalpy changes in compounds, effectively providing a 'zero point' from which all formation reactions are measured.