Question

These questions are not designated as to type or location in the chapter. They may combine several concepts. The following terms are used extensively in thermodynamics. Define each and give an example. (a) exothermic and endothermic (b) system and surroundings (c) specific heat capacity (d) state function (e) standard state (f) enthalpy change, \(\Delta H\) (g) standard enthalpy of formation

Short answer

Defined terms include exothermic/endothermic processes, system/surroundings, specific heat capacity, state function, standard state, enthalpy change, and standard enthalpy of formation with examples.

Step-by-step solution

Define Exothermic and Endothermic

**Exothermic** refers to a process or reaction that releases heat to its surroundings, like the combustion of wood in a fireplace. **Endothermic** refers to a process or reaction that absorbs heat from its surroundings, such as the melting of ice.

Define System and Surroundings

In thermodynamics, the **system** is the specific part of the universe that is of interest, usually the substance or reaction being studied. **Surroundings** are everything outside the system, including the container and air around it.

Define Specific Heat Capacity

**Specific Heat Capacity** is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. For example, water has a high specific heat capacity, which is why it takes a long time to heat up.

Define State Function

A **State Function** is a property that is independent of the path taken to reach a particular state. An example is the internal energy of a system, which depends only on the state and not how it got to that state.

Define Standard State

The **Standard State** is a reference state for a specific substance under standard conditions, which are typically set at 25°C and 1 atm pressure. For gases, it's usually considered to be their behavior as an ideal gas at these conditions.

Define Enthalpy Change ( \( \Delta H \) )

**Enthalpy Change (\(\Delta H\))** is the amount of heat absorbed or released during a chemical reaction at constant pressure. For instance, if \(\Delta H\) is negative, the reaction is exothermic.

Define Standard Enthalpy of Formation

The **Standard Enthalpy of Formation** is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. For example, the formation of water from hydrogen and oxygen gas has a specific standard enthalpy of formation.

Key concepts

Exothermic Reactions

In thermodynamics, understanding energy flow is crucial, and exothermic reactions are a clear demonstration of this. An exothermic reaction is one that releases heat to its surroundings. This release of energy often happens because the total energy of the products is lower than that of the reactants. The classic example of an exothermic process is the combustion of wood. As the wood burns, it releases heat and light, warming the surroundings and illustrating an energy release.

• Characteristics: Heat is released
• Result: Surroundings become warmer
• Example: Combustion of fuels

Exothermic reactions are integral in various everyday applications, from heating homes to powering engines. It's fascinating how such reactions not only change temperature but also create movement, light, and other forms of energy.

Endothermic Reactions

On the flip side, endothermic reactions are those that absorb heat from their surroundings. These processes require energy input to proceed, which results in a cooling effect on the environment. A familiar example is the melting of ice. As ice absorbs heat, it transitions from solid to liquid.

• Characteristics: Heat is absorbed
• Result: Surroundings become cooler
• Example: Melting of ice

These reactions are essential in understanding energy balance in nature and technology, such as in evaporation, photosynthesis, and air conditioning systems. By absorbing heat, endothermic reactions store energy, often converting it into different forms or using it for biological functions.

State Function in Thermodynamics

The concept of a state function is fundamental in thermodynamic studies. A state function refers to a property that depends solely on the current state of the system, not on how it got there. This means its value is determined only by the system's condition at a specific moment in time, such as pressure, temperature, or volume.

• Independence: Unaffected by path taken
• Example: Internal energy, entropy
• Significance: Helps predict state changes

The principle of state functions allows scientists and engineers to predict system behavior without needing to know the details of the process leading to a state. This simplification makes thermodynamic calculations more practical and feasible in analyzing different systems.

Enthalpy Change

Enthalpy change (\(\Delta H\)) is a pivotal concept in thermodynamics and chemistry. It represents the heat absorbed or released during a chemical reaction at constant pressure. When the enthalpy change is negative, the reaction is exothermic, signifying energy release. Conversely, a positive \(\Delta H\) indicates an endothermic reaction, where energy is absorbed.

• Formula: \(\Delta H = H_{final} - H_{initial}\)
• Negative \(\Delta H\): Exothermic, energy released
• Positive \(\Delta H\): Endothermic, energy absorbed

Understanding enthalpy change helps in assessing the thermal energy involved in chemical processes. This information is vital when considering reaction feasibility, safety, and conditions necessary for optimal reaction progress. Enthalpy change data supports engineers and chemists in designing and scaling industrial processes efficiently.