## What is Energy

The term** energy **is very very broad and it has many definitions. Technically,

**energy**is a

**scalar physical quantity**that is associated with the state of one or more objects. Energy is generally defined as the

**potential to do work**

**or produce heat**. Sometimes it is like the “currency” for performing work. You must have energy to accomplish work. To do 1 kilojoule of work, you must expend 1 kilojoule of energy. It must be added, this interpretation can be misleading because energy is not necessarily available to do work.

One of the most wonderful properties of the universe is that **energy** **can be transformed** from one type to another and **transferred** from one object to another. Moreover, when transformed from one type to another and transferred from one object to another, the **total amount of energy is always the same**. It is one of the elementary properties of the universe.

For example, burning gasoline to power cars is an energy conversion process we rely on. The **chemical energy** in gasoline is** converted** to** thermal energy**, which is then converted to **mechanical energy** that makes the car move. The **mechanical energy** has been converted to **kinetic energy**. When we use the brakes to stop a car, that** kinetic energy** is converted by friction back to heat, or **thermal energy**.

## Energy Units

**Energy**is generally defined as the potential to do work or produce heat. This definition causes the SI unit for energy is the same as the unit of work – the

**joule (J)**. Joule is a derived unit of energy and it is named in honor of

**James Prescott Joule**and his experiments on the mechanical equivalent of heat. In more fundamental terms, 1 joule is equal to:

**1 J = 1 kg.m ^{2}/s^{2}**

Since energy is a fundamental physical quantity and it is used in various physical and engineering branches, there are many units in physics and engineering. These units are summarized in following points:

- 1 joule = 0.239 Calories
- 1 joule = 9.48 x 10
^{-4}BTU - 1 joule = 2.778 x 10
^{-7}kWh

**Examples of Energy of 1 Joule:**

One joule in everyday life and in science corresponds to approximately:

- The kinetic energy of an object with mass 1 kg moving at √2 ≈ 1.4 m/s.
- The kinetic energy of a 50 kg object (e.g. human) moving very slowly – approximately 0.72 km/h.
- The energy required to lift a medium-size apple (100 g) 1 meter vertically from the surface of the Earth.
- The heat required to raise the temperature of 1 g of water by 0.24 °C.
- The heat required to evaporate of 0.00044 g of liquid water at 100°C.
- The amount of electricity required to light a 1 watt LED for 1 s.
- Is released by approximately
**3.1****⋅****10**^{10}**fissions**in a nuclear reactor.

**Calorie (unit: cal)**. Calorie is a traditional unit of heat. It is part of the

**International System of Units**(SI). It is defined to be the amount of heat that must be absorbed by 1 gram of water to raise its temperature by 1 °C. Its counterpart in the British Imperial system of units is the BTU, which is defined as the amount of heat required to raise the temperature of one pound of water by one degree Fahrenheit. But we have to distinguish between small calorie and large calorie. The large calorie (unit: Cal) is defined in terms of the kilogram rather than the gram. It is equal to 1000 small calories and it is i.e. 1 kilocalorie (unit: kcal). It is used by nutritionists to characterize the energy-producing potential in food.

- 1 calorie = 4.184 J
- 1 calorie = 0.00397 BTU
- 1 calorie = 1.16 x 10
^{-6}kWh

**British Thermal Unit (unit: BTU)**. British Thermal Unit is a traditional unit of heat. It is part of the British Imperial system of units. It is defined to be the amount of heat that must be absorbed by a 1 one pound of water to raise its temperature by 1 °F at the temperature that water has its greatest density (approximately 39 degrees Fahrenheit). Its counterpart in the

**International System of Units**(SI) is the calorie, which is defined as the amount of heat required to raise the temperature of one gram of water by one degree Celsius.

- 1 British Thermal Unit (BTU) = 1055 J
- 1 British Thermal Unit (BTU) = 252 calories
- 1 British Thermal Unit (BTU) = 0.000293 kWh

**Foot-pound force (unit: ft.lbf)**. Foot-pound force is a derived unit of work and energy. It is equal to the energy transferred to an object when a force of one pound-force (lbf) acts on that object in the direction of its motion through a distance of one foot. The corresponding SI unit is the joule. The foot-pound is often used in ballistics, especially in the United States. Typically muzzle energies of bullets are given in foot-pound force.

- 1 foot-pound force = 1.356 J
- 1 foot-pound force = 0.324 cal
- 1 foot-pound force = 0.00129 BTU

**Kilowatt-hour (unit: kWh)**. Kilowatt-hour is a derived unit of energy. It is used to measure energy, especially electrical energy in commercial applications. One kilowatt-hour is equal to one kilowatt of power produced or consumed over a period of one hour (kilowatts multiplied by the time in hours). The kilowatt hour is commonly used by electric utilities as a billing unit for energy delivered to consumers. 1kW . h = 1kW . 3600s = 3600kWs = 3600kJ = 3600000J. One kilowatt-hour corresponds to the heat required to evaporate of 1.58 kg of liquid water at 100°C. A radio rated at 100 watts operating for 10 hours continuously uses one kilowatt hour.

- 1 kWh = 3.6 x 10
^{6}J - 1 kWh = 8.6 x 10
^{5}cal - 1 kWh = 3412 BTU

**Megawatt-day (unit: MWd)**. Megawatt-day is a derived unit of energy. It is used to measure energy produced, especially in

**power engineering**. One megawatt-day is equal to one megawatt of power produced by power plant over a period of one day (megawatts multiplied by the time in days).

**1 MWd = 24,000 kWh**. At nuclear power plants there are also gigawatt-days, because it approximately corresponds to energy produced by power plant over a period of one day. This unit (MWd) was also used to derive unit of

**fuel burnup**. The most commonly used measure of fuel burnup is the fission energy release per unit mass of fuel. Therefore fuel burnup of nuclear fuel is normally have units of megawatt-days per metric tonne (

**MWd/MTU**), where tonne refers to a metric ton of uranium metal (sometimes MWd/tU HM as Heavy Metal). In this field, the megawatt-day refers to the thermal power of the reactor, not the fraction which is converted to electricity. For example, for a typical nuclear reactor with a thermal power of

**3000 MWth**, about

**~1000MWe**of electrical power is generated in the generator. For example, a reactor with 100 000 kg of fuel operating at 3000MWth power level for 1000 days would have a burnup increase of 30,000 MWd/MTU. In words of fissions, fissioning of about 1 g of U-235 produces about 1 MWd of thermal energy (see: Energy Release per Fission).

- 1 MWd = 8.64 x 10
^{10}J - 1 MWd = 2.06 x 10
^{10}cal - 1 MWd = 8.19 x 10
^{7}BTU

**Electronvolt (unit: eV)**. Electronvolts are a traditional unit of energy particularly in atomic and nuclear physics. Electronvolt is equal to energy gained by a single electron when it is **accelerated** through **1 volt** of **electric potential** difference. The work done on the charge is given by the charge times the voltage difference, therefore the work W on electron is: W = qV = (1.6 x 10^{-19 }C) x (1 J/C) = **1.6 x 10 ^{-19} J**. Since this is very small unit, it is more convenient to use multiples of electronvolts: kilo-electronvolts (keV), mega-electronvolts (MeV), giga-electronvolts (GeV) and so on. Since Albert Einstein showed that mass and energy are

**equivalent and convertible**one into the other, the electronvolt is also a unit of mass. It is common in particle physics, where units of mass and energy are often interchanged, to express mass in units of eV/c

^{2}, where c is the speed of light in vacuum (from E = mc

^{2}). For example, it can be said the

**proton**has mass of

**938.3 MeV**, although strictly speaking it should be

**938.3 MeV/c**. For another example, an electron–positron annihilation occurs when a negatively charged electron and a positively charged positron (each with a mass of 0.511 MeV/c

^{2}^{2}) collide. When an electron and a positron collide, they annihilate resulting in the complete conversion of their rest mass to pure energy (according to the E=mc

^{2}formula) in the form of two oppositely directed 0.511 MeV gamma rays (photons).

**e**^{−}** + e**^{+}** → γ + γ (2x 0.511 MeV)**

- 1 eV = 1.603 x 10
^{-19}J - 1 eV = 3.83 x 10
^{-20}cal - 1 eV = 1.52 x 10
^{-22}BTU

**Example of Energies in Electronvolts**

**Thermal neutrons**are neutrons in thermal equilibrium**with a surrounding medium of temperature 290K (17 °C or 62 °F)**. Most probable energy at 17°C (62°F) for Maxwellian distribution is**0.025 eV**(~2 km/s).- Thermal energy of a molecule is at room temperature about
**0.04 eV**. - Approximately
**1 eV**corresponds to an**infrared photon**of wavelength 1240 nm. - Visible light photons have energies in range 1.65 eV (red) – 3.26 eV (violet).
- The first resonance in n +
^{238}U reaction is**at 6.67 eV**(energy of incident neutron), which corresponds to the first**virtual level in**^{239}**U**, has a total width of only 0.027 eV, and the mean life of this state is 2.4×10^{-14}s. - Ionization energy of atomic hydrogen is
**13.6 eV**. - Carbon-14 decays into nitrogen-14 through beta decay (pure beta decay). The emitted beta particles have a maximum energy of 156 keV, while their weighted mean energy is
**49 keV**. - High energy diagnostic medical x-ray photons have kinetic energies of about
**200 keV.** **Thallium 208,**which is one of nuclides in thedecay chain,^{232}U**emits****gamma rays****of 2.6 MeV which are very energetic and highly penetrating.**- Typical kinetic energy of
**alpha particle**from radioactive decay is about**5 MeV**. It is caused by the mechanism of their production. **The total energy released**in a reactor is**about 210 MeV**per^{235}U fission, distributed as shown in the table. In a reactor,**the average recoverable energy**per fission is**about 200 MeV**, being the total energy minus the energy of the energy of antineutrinos that are radiated away.- Cosmic ray can have energies of
**1 MeV – 1000 TeV**.

## Examples of Energy of 1 Joule

**One joule**in everyday life and in science corresponds to approximately:

- The kinetic energy of an object with mass
**1 kg**moving at √2 ≈**1.4 m/s**. - The kinetic energy of a
**50 kg**object (e.g. human) moving very slowly – approximately**0.72 km/h**. - The energy required to lift a medium-size apple (
**100 g**)**1 meter vertically**from the surface of the Earth. - The heat required to raise the temperature of
**1 g of water by 0.24 °C**. - The heat required to
**evaporate**of**0.00044 g of liquid water**at 100°C. - The amount of electricity required to light a
**1 watt LED**for**1 s**. - Is released by approximately
**3.1****⋅****10**^{10}**fissions**in a nuclear reactor.

## Forms of Energy

**mechanical energy**that is classically divided into

**kinetic**and

**potential energy**. The kinetic energy is related to the velocity of a

**moving object**. The potential energy is related to an

**object’s position**in a

**force field**(gravitational, electric or magnetic). Tension in a spring or surface film tension are other forms of potential mechanical energy (elastic energy). There are many other forms of energy including electrical, magnetical, chemical, and

**nuclear energy**.

**In thermodynamics** the concept of energy is broadened to account for other observed changes. Thermodynamics deals with another type of energy called “**thermal energy**” or “**internal energy**”. The only ways the energy of a closed system can be changed are through transfer of energy **by work** or **by heat**. Further, based on the experiments of Joule and others, a fundamental aspect of the energy concept is that **energy is conserved. **This principle is known as **the first law of thermodynamics**. In general energy is a fundamental concept of thermodynamics and one of the most significant aspects of engineering analysis.

**mechanical energy**(E

_{mech}) is the energy associated with the

**motion**and

**position**of an object usually in some force field (e.g. gravitational field).

**Mechanical energy**(and also the thermal energy) can be separated into two categories, transient and stored. Transient energy is energy in motion, that is, energy being transferred from one place to another. Stored energy is the energy contained within a substance or object. Transient mechanical energy is commonly referred to as

**work**. Stored mechanical energy exists in one of two forms:

**kinetic**or

**potential.**

**The kinetic energy,**, is defined as the energy stored in an object because of its motion. An object in motion has the ability to do work and thus can be said to have energy. It is called kinetic energy, from the Greek word kinetikos, meaning “motion.”

*K*The **kinetic energy** depends on the speed of an object and is the ability of a moving object to do work on other objects when it collides with them. On the other hand, the kinetic energy of an object represents the amount of energy required to increase the velocity of the object from rest (v = 0) to its final velocity. The kinetic energy also depends linearly on the mass, which is a numerical measure of object’s **inertia **and the measure of an object’s resistance to acceleration when a force is applied.

We define the quantity:

**K = ½ mv ^{2}**

to be the **translational kinetic energy** of the object. It must be added, it is called the “translational” kinetic energy to distinguish it from rotational kinetic energy

**Potential energy**, U, is defined as the

**energy stored**in an object subjected to a conservative force. Common types include the

**gravitational potential energy**, the

**elastic potential energy**of an extended spring, and the

**electric potential energy**of an electric charge in an electric field and so on.

In classical mechanics, the gravitational potential energy (U) is energy an object possesses because of its position in a gravitational field. Gravitational potential (V; the gravitational energy per unit mass) at a location is equal to the work (energy transferred) per unit mass that would be needed to move the object from a fixed reference location to the location of the object. The most common use of gravitational potential energy is for an object near the surface of the Earth where the gravitational acceleration can be assumed to be constant at about 9.8 m/s^{2}.

**U = mgh**

**internal energy**(also called the

**thermal energy**) is defined as the energy associated with

**microscopic forms of energy**. It is an extensive quantity, it depends on the size of the system, or on the amount of substance it contains. The SI unit of

**internal energy**is the

**joule (J)**. It is the energy contained within the system, excluding the kinetic energy of motion of the system as a whole and the potential energy of the system.

**Microscopic forms of energy**include those due to the

**rotation**,

**vibration, translation**, and

**interactions**among the molecules of a substance. None of these forms of energy can be measured or evaluated directly, but techniques have been developed to evaluate the change in the total sum of all these microscopic forms of energy.

In addition, energy is can be stored in the chemical bonds between the atoms that make up the molecules. This energy storage on the atomic level includes energy associated with electron orbital states, nuclear spin, and binding forces in the nucleus.

**enthalpy**is a measurement of energy in a thermodynamic system. It is the thermodynamic quantity equivalent to the total heat content of a system. The

**enthalpy**is defined to be the sum of the internal energy

**E**plus the product of the pressure

**p**and volume

**V.**In many thermodynamic analyses the sum of the internal energy U and the product of pressure p and volume V appears, therefore it is convenient to give the combination a name, enthalpy, and a distinct symbol, H.

The enthalpy is the preferred expression of system energy changes in many chemical, biological, and physical measurements **at constant pressure**. It is so useful that it is tabulated in the **steam tables** along with specific volume and specific internal energy. It is due to the fact, it **simplifies the description of energy transfer**. At constant pressure, the enthalpy change equals the energy transferred from the environment through heating **(Q = H _{2} – H_{1})** or work other than expansion work. For a variable-pressure process, the difference in enthalpy is not quite as obvious.

**entropy**is a quantitative measure of disorder, or of the energy in a system to do work.

In statistical physics, entropy is a measure of the disorder of a system. What disorder refers to is really the **number of microscopic configurations**, **W**, that a thermodynamic system can have when in a state as specified by certain macroscopic variables (volume, energy, pressure, and temperature). By “microscopic states”, we mean the exact states of all the molecules making up the system.

Mathematically, the exact definition is:

**Entropy = (Boltzmann’s constant k) x logarithm of number of possible states**

**S = k _{B} logW**

This equation, which relates the microscopic details, or microstates, of the system (via *W*) to its macroscopic state (via the **entropy S**), is the key idea of statistical mechanics. In a closed system, entropy never decreases, so in the Universe entropy is irreversibly increasing. In an open system (for example, a growing tree), entropy can decrease and order can increase, but only at the expense of an increase in entropy somewhere else (e.g. in the Sun).

**Gibbs free energy**is a thermodynamic potential that is defined as the enthalpy of the system minus the product of the temperature times the entropy of the system. Since the

**enthalpy**is defined to be the sum of the internal energy

**E**plus the product of the pressure

**p**and volume

**V.**

**nuclear power plant**has an electric-generating capacity of

**1000 MWe**. It produces 1 000 000 000 joules of electrical energy per second. The heat source in the nuclear power plant is a

**nuclear reactor**. As is typical in all conventional thermal power stations the heat is used to generate steam which drives a

**steam turbine**connected to a generator which produces electricity. The turbines are heat engines and are subject to the efficiency limitations imposed by the

**second law of thermodynamics**. In modern nuclear power plants the overall thermodynamic efficiency is about

**one-third**(33%), so

**3000 MWth**of thermal power from the fission reaction is needed to generate

**1000 MWe**of electrical power.

Since **voltage** is **electric potential energy** per unit charge, the **Kirchhoff’s voltage law** can be seen to be a consequence of **conservation of electrical energy**. **Kirchhoff’s voltage law states:**

*The algebraic sum of the voltages (drops or rises) encountered in traversing any loop of a circuit in a specified direction must be zero.*

The algebraic sum of the voltages (drops or rises) encountered in traversing any loop of a circuit in a specified direction must be zero.

Simply, the voltage changes around any closed loop must sum to zero. The sum of the **voltage rises** is equal to the sum of the** voltage drops** in a loop. No matter what path you take through an electric circuit, if you return to your starting point you must measure the same voltage, constraining the net change around the loop to be zero. This rule is equivalent to saying that each point on a mountain has only one elevation above sea level. If you start from any point and return to it after walking around the mountain, the algebraic sum of the changes in elevation that you encounter must be zero.

**radiant energy**is the energy of

**electromagnetic**and

**gravitational radiation**. The term “

**radiant energy**” is most commonly used in the fields of radiometry, solar energy, heating and lighting. As energy, its SI unit is the

**joule (J)**. The quantity of radiant energy may be calculated by integrating radiant flux with respect to time.

**Radiant heat transfer**is very important in power industry, because it is one of the most important ways , how thermal energy can be transferred. It does not need a medium, such as air or metal, to take place. Any material that has a temperature above absolute zero gives off some radiant energy. Most energy of this type is in the infra-red region of the electromagnetic spectrum although some of it is in the visible region.

**Radiant heat transfer** rate from a body (e.g. a black body) to its surroundings is proportional to the **fourth power** of the absolute temperature and can be expressed by the following equation:

*q = εσT ^{4}*

where** σ** is a fundamental physical constant called the **Stefan–Boltzmann constant**, which is equal to** 5.6697×10 ^{-8} W/m^{2}K^{4}**. This relationship is called the

**Stefan–Boltzmann law**. The

**emissivity, ε**, of the surface of a material is its effectiveness in emitting energy as thermal radiation and varies between 0.0 and 1.0. By definition, a black body in thermal equilibrium has an emissivity of

*ε*= 1.0. It can be seen, radiation heat transfer is important at very high temperatures and in a vacuum.

Two bodies that radiate toward each other have a net heat flux between them. The net flow rate of heat between them is given by:

**Q = εσA _{1-2}(T^{4}_{1} −T^{4}_{2}) [J/s]**

**q = εσ(T ^{4}_{1} −T^{4}_{2}) [J/m^{2}s]**

The area factor A_{1-2}, is the area viewed by body 2 of body 1, and can become fairly difficult to calculate.

**Ionization energy**, also called

**ionization potential**, is the energy necessary to

**remove an electron**from the neutral atom.

X + energy → X^{+} + e^{−}

where X is any atom or molecule capable of being ionized, X^{+} is that atom or molecule with an electron removed (positive ion), and e^{−} is the removed electron.

There is an ionization energy for each successive electron removed. The electrons that circle the nucleus move in fairly well-defined orbits. Some of these electrons are more tightly bound in the atom than others. For example, only 7.38 eV is required to remove the outermost electron from a lead atom, while 88,000 eV is required to remove the innermost electron.

**Ionization energy**is lowest for the alkali metals which have a single electron outside a closed shell.**Ionization energy**increases across a row on the periodic maximum for the noble gases which have closed shells.

For example, sodium requires only 496 kJ/mol or 5.14 eV/atom to ionize it. On the other hand neon, the noble gas, immediately preceding it in the periodic table, requires 2081 kJ/mol or 21.56 eV/atom.

The ionization energy associated with removal of the first electron is most commonly used. The *n*th ionization energy refers to the amount of energy required to remove an electron from the species with a charge of (*n*-1).

1st ionization energy

X → X^{+} + e^{−}

2nd ionization energy

X^{+} → X^{2+} + e^{−}

3rd ionization energy

X^{2+} → X^{3+} + e^{−}

For example, only 7.38 eV is required to remove the outermost electron from a lead atom, while 88,000 eV is required to remove the innermost electron.

**Nuclear energy**comes either from spontaneous nuclei conversions or induced nuclei conversions. Among these conversions (nuclear reactions) belong for example nuclear fission, nuclear decay and nuclear fusion. Conversions are associated

**with mass and energy changes**. One of the striking results of

**Einstein’s theory of relativity**is that

**mass and energy are equivalent and convertible**, one into the other. Equivalence of the mass and energy is described by Einstein’s famous formula:

## Mass-energy Equivalence

**Einstein’s theory of relativity**is that

**mass and energy are equivalent and convertible**, one into the other. Equivalence of the mass and energy is described by Einstein’s famous formula:

, where M is the small amount of mass and C is the speed of light.

What that means? If the nuclear energy is generated (splitting atoms, nuclear fusion), a small amount of mass (saved in the **nuclear binding energy**) transforms into the pure energy (such as kinetic energy, thermal energy, or radiant energy).

The energy equivalent of one gram (1/1000 of a kilogram) of mass is equivalent to:

**89.9 terajoules****25.0 million kilowatt-hours (≈ 25 GW·h)****21.5 billion kilocalories (≈ 21 Tcal)****85.2 billion BTUs**

or to the energy released by combustion of the following:

**21.5 kilotons of TNT-equivalent energy (≈ 21 kt)****568,000 US gallons of automotive gasoline**

Any time energy is generated, the process can be evaluated from an **E = mc**** ^{2 }**perspective.

## Principle of Conservation of Energy

**energy can be transformed from one type to another**and

**transferred from one object to another**. Moreover, when transformed from one type to another and transferred from one object to another, the

**total amount of energy is always the same**. It is one of the elementary properties of the universe.

**In thermodynamics** the concept of energy is broadened to account for other observed changes, and the **principle of conservation of energy** is extended to include a wide variety of ways in which systems interact with their surroundings. The only ways the energy of a closed system can be changed are through transfer of energy **by work** or **by heat**. Further, based on the experiments of Joule and others, a fundamental aspect of the energy concept is that **energy is conserved. **This principle is known as **the first law of thermodynamics**. The first law of thermodynamics can be written in various forms:

**In words:**

**Equation form:**

**∆E**_{int}** = Q – W**

where **E _{int }**represents the

**internal energy**of the material, which depends only on the

**material’s state**(temperature, pressure, and volume).

**Q**is the

**net heat added**to the system and

**W**is the

**net work done by**the system. We must be careful and consistent in following the sign conventions for Q and W. Because W in the equation is the work done by the system, then if work is done on the system, W will be negative and E

_{int}will increase.

Similarly, Q is positive for heat added to the system, so if heat leaves the system, Q is negative. This tells us the following: The **internal energy** of a system tends to increase if heat is absorbed by the system or if positive work is done on the system. Conversely, the internal energy tends to decrease if heat is lost by the system or if negative work is done on the system. It must be added Q and W are path dependent, while E_{int} is path independent.

**Differential form:**

**dE _{int} = dQ – dW**

The internal energy E_{int} of a system tends to increase if energy is added as heat Q and tends to decrease if energy is lost as work W done by the system.

## Energy Sources

**Energy sources** have always played a very important role in the development of human society. Since the industrial revolution the energy has been a driving force for the modern civilization development. Technological development and **consumption of primary energy**, along with the increase of the world population are interdependent. In past 20 years, the world around us has changed significantly. Technology has become one of the main drivers of economic and social development. The rapid advancement of Information Technology (IT) all over the world has transformed not only the way we think, but also the way we act. It must be noted that practically all technologies run on **electrical energy** and therefore the share of electricity is increasing rapidly, faster than **Total Primary Energy Supply** (TPES – the sum of production and imports subtracting exports and storage changes.).

At present, fossil fuel is still the world’s predominant energy source and its extraction, production and use are not considered to be efficient regardless of the new technologies available to improve its use and extraction. When studying energy resources, we have to distinguish the **primary energy sources** and **secondary energy sources**.

## Primary Energy Sources

**Primary energy (PE)** is an energy resource found in nature that has not been subjected to any conversion or transformation process. It is energy contained in **raw fuels**, and other forms of energy received as input to a system. Primary energy sources take many forms, including nuclear energy, fossil energy — like oil, coal and natural gas — and renewable sources like wind, solar, geothermal and hydropower. These primary sources **can be converted** to secondary energy source, so called **energy carriers**. Primary energy sources can be divided into:

- Non-renewable sources
- Fossil fuels
- Oil
- Coal
- Natural gas

- Mineral fuels
- Natural Uranium
- Natural Thorium

- Fossil fuels
- Renewable sources
- Solar energy
- Wind energy
- Hydro and tidal energy
- Geothermal energy
- Biomass energy (if sustainably exploited)

## Secondary Energy Sources – Energy Carriers

**Secondary energy sources**, also called

**energy carriers**, are derived from the transformation of primary energy sources. They are called energy carriers, because they move energy in a useable form from one place to another. The well-known energy carriers are:

**Electricity****Petrol****Hydrogen**

**Electricity** and **hydrogen** made from primary energy sources such as coal, natural gas, nuclear energy, petroleum, and renewable energy sources. Electricity is particularly useful since it has **low entropy** (is highly ordered) and can be converted into other forms of energy very efficiently. Simply, we cannot say that hydrogen have potential to offset fossil fuels.

Secondary energy sources are used, because its using is easier than using a primary energy source. For example, using electricity for lighting is safer than using petroleum in candles or kerosene lamps.

On the other hand any conversion of primary energy to energy carrier is associated with some inefficiency. Therefore when dealing with secondary energy source, we have to always consider the way, how the carrier was made.

**Reactor Physics and Thermal Hydraulics:**

- J. R. Lamarsh, Introduction to Nuclear Reactor Theory, 2nd ed., Addison-Wesley, Reading, MA (1983).
- J. R. Lamarsh, A. J. Baratta, Introduction to Nuclear Engineering, 3d ed., Prentice-Hall, 2001, ISBN: 0-201-82498-1.
- W. M. Stacey, Nuclear Reactor Physics, John Wiley & Sons, 2001, ISBN: 0- 471-39127-1.
- Glasstone, Sesonske. Nuclear Reactor Engineering: Reactor Systems Engineering, Springer; 4th edition, 1994, ISBN: 978-0412985317
- Todreas Neil E., Kazimi Mujid S. Nuclear Systems Volume I: Thermal Hydraulic Fundamentals, Second Edition. CRC Press; 2 edition, 2012, ISBN: 978-0415802871
- Zohuri B., McDaniel P. Thermodynamics in Nuclear Power Plant Systems. Springer; 2015, ISBN: 978-3-319-13419-2
- Moran Michal J., Shapiro Howard N. Fundamentals of Engineering Thermodynamics, Fifth Edition, John Wiley & Sons, 2006, ISBN: 978-0-470-03037-0
- Kleinstreuer C. Modern Fluid Dynamics. Springer, 2010, ISBN 978-1-4020-8670-0.
- U.S. Department of Energy, THERMODYNAMICS, HEAT TRANSFER, AND FLUID FLOW. DOE Fundamentals Handbook, Volume 1, 2 and 3. June 1992.

## Social Media