Question

(a) What is meant by the term standard conditions with reference to enthalpy changes? (b) What is meant by the term enthalpy of formation? (c) What is meant by the term standard enthalpy of formation?

Short answer

(a) Standard conditions for enthalpy changes refer to a set of physical conditions (pressure of 100 kPa and temperature of 298.15 K) under which thermodynamic quantities are measured, ensuring consistent comparisons between experiments. (b) Enthalpy of formation (ΔHf) is the heat absorbed or released during the formation of one mole of a species from its constituent elements in their most stable states at a specific temperature and pressure. (c) Standard enthalpy of formation (ΔHf°) is the enthalpy change when one mole of a compound is formed from its constituent elements in their most stable states at standard conditions (100 kPa and 298.15 K). It helps predict reaction energetics and determine the direction of a reaction.

Step-by-step solution

(a) Define standard conditions

The standard conditions, in the context of enthalpy changes, refer to a set of physical conditions under which thermodynamic quantities are measured or experimentally determined. It ensures that results from different experiments can be consistently compared. The standard conditions typically include a pressure of 100 kPa (1 atm) and a temperature of 298.15 K (25°C).

(b) Define enthalpy of formation

The enthalpy of formation, written as ΔHf, is the amount of heat absorbed or released during the formation of a single species (one mole) from its constituent elements in their most stable states at a specified temperature and pressure. The enthalpy of formation is a measure of the stability of the compound and has a direct impact on the spontaneity of a chemical reaction.

(c) Define the standard enthalpy of formation

The standard enthalpy of formation, written as ΔHf°, is the enthalpy change that occurs when one mole of a compound is formed from its constituent elements in their most stable states at standard conditions (a pressure of 100 kPa and a temperature of 298.15 K). This value helps in comparing the relative enthalpy changes during the formation of different compounds under the standard conditions, enabling chemists to predict reaction energetics and determine the direction in which a reaction is more likely to proceed.

Key concepts

Standard Conditions

Standard conditions are crucial when discussing and measuring enthalpy changes in chemistry. They provide a consistent reference point, ensuring that when scientists report energy changes, they are speaking the same language. These conditions typically mean a pressure of 100 kPa, which is equivalent to 1 atmosphere (atm), and a temperature of 298.15 Kelvin (K), or 25 degrees Celsius (°C).
- These standard conditions ensure that different experiments' results are comparable. - It allows chemists to make accurate predictions and comparisons between different substances and reactions.
Under standard conditions, discrepancies due to variations in laboratory settings are minimized, paving the way for a uniform understanding of thermodynamic properties across different studies.

Enthalpy of Formation

The enthalpy of formation, represented by the symbol ΔHf, is an essential concept in thermochemistry. It represents the heat change associated with the formation of 1 mole of a compound from its basic elements in their standard, most stable state.
- The value of ΔHf can help determine whether heat is released (exothermic) or absorbed (endothermic) during this formation. - By gauging the enthalpy of formation, chemists can assess the energy stability of compounds.
For instance, when hydrogen gas and oxygen gas combine to form water, the enthalpy of formation would quantify the energy change in this reaction. If the ΔHf is negative, it indicates that forming the compound releases energy, implying the compound is more stable compared to its separate elements.

Standard Enthalpy of Formation

The standard enthalpy of formation, noted as ΔHf°, extends the concept of enthalpy of formation with the inclusion of standard conditions. It quantifies the energy change when one mole of a substance forms from its elements in their most stable forms, measured precisely at the accepted standard conditions of 100 kPa and 298.15 K.
- Standard enthalpy of formation values help chemists compare reaction energetics under controlled conditions. - They are crucial for calculating the overall enthalpy changes in multi-step reactions through Hess's law.
For example, the standard enthalpy of formation of water allows chemists to determine and understand energy changes involved in its formation, compared alongside other compounds under identical conditions. Such data is invaluable for predicting reaction behavior and enthusing insights into energy efficiency and feasibility.