Table of Contents

## Hess’s Law (Hess´s Law of Constant Heat Summation)

### Definition

Hess’s Law, also known as Hess’s Law of Constant Heat Summation, stated that no matter how many steps or stages are present in a reaction, the total enthalpy change for the entire reaction is the sum of each individual change. Enthalpy is a thermodynamic measurement assessing the total heat content of a system. It is equivalent to the internal energy of the system plus the product of the pressure and volume as stated below.

**H = U + pV**

H = enthalpy of the system

U = internal energy of the system

p = pressure of the system

V = volume of the system

Let us look at a reaction: A → B → C. Here, a substance A is undergoing a reaction to become B which then undergoes another reaction to become C. The change in enthalpy of the energy change is denoted by ΔH.

The ΔH for the total reaction is equal to the sum of the ΔH for the first reaction plus the ΔH for the second reaction.

**ΔH _{A͢͢͢͢͢ to B} + ΔH_{B to C} = ΔH_{A to C}**

** ****Calculation Using Hess’s Law**

Let us see how to understand the actual calculation that takes place in a reaction. Look at the reaction below:

**CH _{4} + 2O_{2} → CO_{2} + 2H_{2}O**

Here, methane and oxygen react to form carbon dioxide and water. In order for the reaction to occur, the elements need to be rearranged. This is done be breaking bonds and forming new bonds between elements.

CH_{4} (methane) needs to be broken down into its simple elements: C (carbon) and H (hydrogen). When this occurs, energy change occurs which is referred to as: (ΔH_{f})_{CH4}. This is the standard energy of formation referring to standard elements present in nature. For O_{2} (oxygen), we do not need to break it into individual O elements since in nature, single O isn’t present. Standard form is O_{2}. In order to form the products, C and O have to combine to form CO_{2} (carbon dioxide) and H and O have to combine to form H_{2}O (water). The enthalpies for formation for these two products are: (ΔH_{f})_{CO2} and (ΔH_{f})_{H2O}, respectively.

The total enthalpy of the entire reaction would be as follows:

**ΔH _{reaction} = (ΔH_{f})_{CO2} + 2(ΔH_{f})_{H2O} – (ΔH_{f})_{CH4}**

The minus sign for the enthalpy for methane is due to the breakup of the bonds that are taking place.

## Gibb’s Free Energy** **

### Definition

Gibb’s Free Energy is the energy that is associated with a chemical reaction that can be utilized to perform work. It conveys the amount of free energy exists for a reaction to go forward. In general, a reaction wants to minimize energy use (enthalpy) and maximize entropy. Entropy is interpreted as the degree of disorder or randomness that exists in a system. The calculation of the Gibb’s Free Energy (ΔG) can tell if the reaction can occur spontaneously or not.

Enthalpy change (ΔH) and entropy change (ΔS) are competing events. Enthalpy wants to be minimal in a reaction whereas entropy wants to be maximal in a reaction. Also, entropy is associated with temperature since the disorder that exists in a system is dependent on temperature. The higher the temperature, the more the disorder that is present.

The relationship between the Gibb’s Free Energy (ΔG), enthalpy change (ΔH), and entropy change (ΔS) is as follows:

**ΔG = ΔH – T ΔS**

Note the negative sign since enthalpy and entropy are opposing reaction concepts. Also, temperature (T) is measured in Kelvin (K).

**To Be Spontaneous or Not To Be Spontaneous, That is the Question?**

The reaction that needs to take place can occur spontaneously (favorably) or non-spontaneously (unfavorably). This is determined by the calculation of the Gibb’s Free Energy (ΔG).

If ΔG < 0, then the reaction is considered to be a spontaneous reaction.

If ΔG > 0, then the reaction is considered to be a non-spontaneous reaction.

Understand that even if the reaction is exothermic (requires no energy input), it might not happen if it lowers the entropy too much. Also, just because something is spontaneous, it does not mean it is quick. Reactions are either spontaneous (favorable) or non-spontaneous (unfavorable). The reaction can also be quick or slow. Both of these concepts are not directly related since they depend on different properties of the reaction.

## Coefficient** of Thermal Expansion**** **

### Definition

The coefficient of thermal expansion describes how the size of different types of matter can be affected (changed) by a change in temperature. This change can be associated with linear (one-dimensional) change or with volumetric (three-dimensional) change. When an object is heated (implying temperature is increasing), the heated object is larger. Increasing heat will continue causing some expansion to occur based on degree Kelvin change in temperature.

### Linear Thermal Expansion

An object has a linear dimension which when heated undergoes linear expansion. This change in thermal expansion in the linear (one-dimensional) direction is denoted as follows:

**L _{final} = L_{initial} (1 + α ΔT)**

L_{final} = final length

L_{initial} = initial length

α = coefficient of linear expansion

ΔT = temperature change

The coefficient of linear expansion, α = 1 / temperature. Thus, the units for α are 1 / Kelvin.

### Volumetric Thermal Expansion

An object has a volumentric dimension which when heated undergoes volumetric expansion. This change in thermal expansion in the volumetric (three-dimensional) direction is denoted as follows:

**V _{final} = V_{initial} (1 + α_{v} ΔT)**

V_{final} = final volume

V_{initial} = initial volume

α_{v} = coefficient of volumetric expansion

ΔT = temperature change

The coefficient of volumetric expansion, α_{v} = 3 α. This is because the volumetric coefficient is associated with three dimensions, thus, it is equal to three of the coefficient of linear expansions.

### Simplifying Thermal Expansion Calculations** **

The thermal expansion equations for linear expansion and volumetric expansion can be stated in a different manner based on change in length and change in volume, respectively.

**Linear Expansion**

**L _{final} = L_{initial} (1 + α ΔT)**

**L _{final} = L_{initial} + (L_{initial} α ΔT)**

**L _{final} = L_{initial} + ΔL**

So, the change in length, ΔL = L_{initial} α ΔT.

### Volumetric Expnasion

**V _{final} = V_{initial} (1 + α_{v} ΔT)**

**V _{final} = V_{initial} + (L_{initial} α_{v} ΔT)**

**V _{final} = V_{initial} + ΔL**

So, the change in volume, ΔV = V_{initial} α_{v} ΔT.