Kinetic energy is the cause of temperature, and heat in the atmosphere.

Author; Rogelio Pérez C

Summary;

At present there exists a world problem known as climate change, which consists of an increase in the temperature of the planet, and as science shows that the temperature and heat of any system are given by the kinetic energies of the atoms or molecules that make up its systems, then this work explains that the cause of the increase in the temperature of the atmosphere, is due to the increase in the kinetic energy of its gas molecules, measuring the difference in the kinetic energy of the atmospheric gas molecules when they are at 14°C and 15°C, it seems simple, logical and that it has nothing special, but that the point where we are today, because the temperature of the atmosphere is explained in another way, “greenhouse effect”,  is explained, because the only way to measure the temperature and heat of any system, is with the kinetic energy of the atoms or molecules that compose it, this work is not responding that causes the kinetic energy in the gas molecules of the atmosphere. which I have already explained in other blog. Currently the theory of the greenhouse effect uses the infrared radiation of the surface of the earth, and an exotic characteristic of heat retention or infrared of certain gases in the atmosphere, to explain to us temperature, heat and the cause of both.

Introduction

The world is currently implementing a strategy to deal with a climate problem, which consists of an increase in the temperature of the atmosphere, which consists in the reduction of gases in the atmosphere, called greenhouse gases like CO2, this work is written to review whether the strategy being implemented, is a false solution, based on a bad interpretation of the temperature, because just as an aspirin does not cure aids, nor the reduction of the smaller gases of the atmosphere, is the best strategy to combat its temperature. The problem of continuing with this strategy is that besides not working, end the most harmed will always be the people is that as in the case of hen and pig when making a scramble of eggs with ham, in this case the hen is the governments, and the pig is the people.

The theory of the greenhouse effect currently uses infrared radiation from the surface of the earth to explain temperature, heat, and the cause of both. Infrared radiation is not the cause of kinetic energy in the atmosphere, because 99.9% of the molecules in the atmosphere do not absorb infrared, but if they emit infrared, so that the absorption of infrared is not a cause to emit it, for those who still believe in the miracle that a mass of 0.04% of a system, They are the main cause of transferring heat to 99.9% of the remaining mass, take a calculator and with this heat equation, q=m×C×ΔT, Calculate whether this small mass can influence another larger mass. finally if the absorption of infrared by GHG, can transfer enough heat to increase the kinetic energy of the atmosphere, this would make the atmosphere self-sufficient energetically, and with unstoppable heat, Because GHG would transfer heat to the rest of the atmosphere, and the rest of the atmosphere would transfer infrared to GHG and vice versa.

In this work it will measure the difference in the kinetic energy of the molecules that make up the atmosphere, when they have a temperature of 14°C and 15°C, to show that the increase in the temperature of the atmosphere is reflected in an increase in the kinetic energies of their molecules.

Theory statement and definitions

The greenhouse effect theory

The greenhouse effect is a process in which thermal radiation emitted by the planetary surface is absorbed by atmospheric greenhouse gases (GHGs) and radiated in all directions. As part of this radiation is returned to the Earth's surface and lower atmosphere.1

Kinetic of gases theory

The kinetic of gases theory is a physical and chemical theory that explains the macroscopic behavior and properties of gases (the law of ideal gases), based on a statistical description of microscopic molecular processes. The kinetic theory was developed based on studies by physicists such as Daniel Bernoulli in the 18th century, Ludwig Boltzmann and James Clerk Maxwell in the late 19th century.2

 

Charles law for gases, for any gas, the ratio between temperature and volume is directly proportional, if the quantity of gas and pressure remain constant.

Mathematically we can express it like this:

Where;

V is the volume

T is the absolute temperature (i.e measured in kelvin).

k is the constant of proportionality.3

Heat, q, is thermal energy transferred from a hotter system to a cooler system that are in contact. Temperature is a measure of the average kinetic energy of the atoms or molecules in the system. The zeroth law of thermodynamics says that no heat is transferred between two objects in thermal equilibrium; therefore, they are the same temperature.4

Heat, is thermal energy transferred from a hotter system to a cooler system that are in contact.

We can calculate the heat released or absorbed using the specific heat capacity C, the mass of the substance, m, and the change in temperature, ΔT in the equation:     q=m×C×ΔT

Heat and temperature are two different but closely related concepts. Note that they have different units: temperature typically has units of degrees Celsius (degrees °C,) or Kelvin (K), and heat has units of energy, Joules (J).

Temperature is a measure of the average kinetic energy of the atoms or molecules in the system. The water molecules in a cup of hot coffee have a higher average kinetic energy than the water molecules in a cup of iced tea, which also means they are moving at a higher velocity.5

Temperature is also an intensive property, which means that the temperature doesn't change no matter how much of a substance you have (as long as it is all at the same temperature!). This is why chemists can use the melting point to help identify a pure substance—minus the temperature at which it melts is a property of the substance with no dependence on the mass of a sample.

The equipartition theorem relates the temperature of a system to its average energies. It makes quantitative predictions, provides the total kinetic and potential energies for a system at a given temperature, from which the heat capacity of the system can be calculated. However, the equipartition also provides the average values of individual energy components, such as the kinetic energy of a particular particle or the potential energy of a single spring. For example, it predicts that each atom in an ideal monoatomic gas has an average kinetic energy of (3/2) k B T in thermal equilibrium, where k B is Boltzmann's constant and Te the temperature (thermodynamics).6

Thermal motion of an α-helical peptide. The jittery motion is random and complex and the energy of any particular atom can fluctuate wildly. Nevertheless, the equipartition theorem allows the average kinetic energy of each atom to be computed, as well as the average potential energies of many vibrational modes. The grey, red and blue spheres represent atoms of carbon, oxygen and nitrogen, respectively; the smaller white spheres represent atoms of hydrogen.7

The mole (symbol: mole) is the unit with which the amount of substance is measured, one of the seven fundamental physical magnitudes of the International System of Units.

In any substance (chemical element or compound) and considering at the same time a certain type of elemental entities that make up it, the mole, mole symbol, is the SI unit of quantity of substance. A mole contains exactly 6,022 140 76 × 10–23 elemental entities.8

Kinetic energy is the energy of a moving body. Kinetic energy is defined as the work to be done by the force it exerts on the resting body to accelerate it.9

Development

To begin, we will find the quadratic mean velocity of each molecule of these 4 gases at a temperature of 15°C; the formula is as follows;

Nitrogen 78%

R= 8.31 J/mol.k

T= 15+273=288 k

M (N2) = 14.0067 + 14.0067 =28 g/mol

             =0.028kg/mol

Vcm= √ (3 *8, 31 *288)/0.028=

Vcm= √ (24.93 *288)/0.028=

Vcm= √7179.8 / 0.028=506.38 m/s

Oxygen 21%

R= 8.31 J/mol.k

T= 15+273=288 k

M (O2) = 16. + 16 =32 g/mol

             =0.032kg/mol

Vcm= √ (3 *8.31 *288)/0.032=

Vcm= √ (24.93 *288)/0.032=

Vcm= √7179.8/ 0.032= 473.67 m/s

Argon 0.934%

R= 8.31 J/mol.k

T= 15+273=288k

M (Ar) = 39.9 =39.9 g/mol

             =0.0399kg/mol

Vcm= √ 3 *8, 31 *288/0.0399=

Vcm= √ (24.93 *288)/0.0399=

Vcm= √ 7179.8 / 0.0399= 424.2 m/s

Carbon dioxide (CO2)

R= 8.31 J/mol.k

T= 15+273=288 k

M(CO2)= 12 + 2*16 =44 g/mol

             =0.044kg/mol

Vcm= √3 *8, 31 *288/0.044=

Vcm= √ (24.93 *288)/0.044=

Vcm= √7179.8 / 0.044= 403, 95 m/s

 

Average quadratic speed of the following molecules at 15°C temperature;
GAS	Vcm. Of molecules  at 15°C
Nitrogen               (N2)	506.38 m/s
Oxygen                 (O2)	473.67 m/s
Argón                    (Ar)	424.20 m/s
Carbon dioxide    (CO2)	403.95 m/s.

As the temperature of the atmosphere is a measure of the average kinetic energy of its molecules, then we will find the kinetic energy for each of the 4 main molecules.

Kinetic energy is a form of energy, known as motion energy. The kinetic energy of an object is the energy produced by its mass-dependant movements and speed of the same. Kinetic energy is usually abbreviated by the letters "EC" or "Ek". The word kinetics is of Greek origin “kinesis” meaning “movement”.

Kinetic energy is represented by the following formula: EC=½ mv². Kinetic energy is measured in Joules (J), mass in kilograms (kg) and velocity in meters over seconds (m/s).4

Nitrogen:

M= 0.028kg/mol

V²= 506.38m/s²

Ec= ½ 0.028kg/ mol(*506.38m/s) ²

Ec=3589.89 J

The kinetic energy (E) of a body with mass m = 0.028 kilograms and velocity v = 506.38 m/s equals 3589.89 J

 

Oxygen

M= 0.032kg/mol

V²= 473.67m/s²

Ec= ½ 0.032kg/ mol*(473.67 m/s) ²

Ec= 3589.81 J

The kinetic energy (E) of a body with mass m = 0.032 kilograms and velocity v = 473.67 m/s equals 3589.81 J

 

Argón

M= 0.0399kg/mol

V²= 424.20m/s

Ec= ½ 0.0399kg/ mol*(424.20 m/s) ²

Ec=3589.92 J

The kinetic energy (E) of a body with mass m = 0.0399 kilograms and velocity v = 424.20 m/s equals 3589.92 J

 

Carbón Dioxide   

M= 0.044kg/mol

V²= 403.95m/s

Ec= ½ 0.044kg/ mol*(403.95 m/s) ²

Ec= 3589.86 J

The kinetic energy (E) of a body with mass m = 0.044 kilograms and velocity v = 403.95 m/s equals 3589.86 J

 

Kinetic energy of each mole of the different gases

GAS	kinetic energy (Heat)  at 15°C
Nitrogen                  (N2)	3589.89 J
Oxygen                  (O2)	3589.81 J
Argón                     (Ar)	3589.92 J
Carbón Dioxide    (CO2)	3589.86 J.

 

Parts per million (ppm) is the unit that is frequently used to measure the volume that occupy small amounts of elements (also called traces) within a mixture.

 

The parts per million of the following gases in the atmosphere
GAS	parts per million
Nitrogen                 (N2)	780.800
Oxygen                    (O2)	209.450
Argón                      (Ar)	9.340
Carbón Dioxide    (CO2)	410

 

 

GAS	VOLUME     PPM	Kinetic energy per Mole gas 15°C	TOTAL(Ek) Mole Gas x Volume 15°C
Nitrogen              (N2)	780.800	3589.89 J	2.802.986.112 J
Oxygen               (O2)	209.450	3589.81 J	751.885.705 J
Argón                  (Ar)	9.340	3589.92 J	33.529.853 J
carbón  Dioxide(CO2)	410	3589.86 J.	1.471.843 J
TOTAL	1.000.000	3589,87 j	3.589.873.512 J

 Now we will find the quadratic mean velocity of each molecule of these 4 gases at a temperature of 14°C;

 

Nitrogen 78%

R= 8.31 J/mol.k

T= 14+273=287 k

M (N2) = 14.0067 + 14.0067 =28 g/mol

             =0.028kg/mol

Vcm= √ (3 *8, 31 *287)/0.028=

Vcm= √ (24.93 *287)/0.028=

Vcm= √7154.9 / 0.028=505.50 m/s

 

Oxygen 21%

R= 8.31 J/mol.k

T= 14+273=287 k

M (O2) = 16. + 16 =32 g/mol

             =0.032kg/mol

Vcm= √ (3 *8.31 *287)/0.032=

Vcm= √ (24.93 *287)/0.032=

Vcm= √7154.9/ 0.032= 472.85 m/s

 

Argon 0.934%

R= 8.31 J/mol.k

T= 14+273=287k

M (Ar) = 39.9 =39.9 g/mol

             =0.0399kg/mol

Vcm= √ 3 *8, 31 *287/0.0399=

Vcm= √ (24.93 *287)/0.0399=

Vcm= √ 7154.9 / 0.0399= 423.46 m/s

 

Carbon dioxide (CO2)

R= 8.31 J/mol.k

T= 14+273=287 k

M (CO2) = 12 + 2*16 =44 g/mol

             =0.044kg/mol

Vcm= √3 *8, 31 *287/0.044=

Vcm= √ (24.93 *287)/0.044=

Vcm= √7154.9 / 0.044= 403, 25 m/s

 

Average quadratic speed of the following molecules at 14°C temperature;
GAS	Vcm. Of molecules  at 14°C
Nitrogen               (N2)	505.50 m/s
Oxygen                 (O2)	472.85 m/s
Argón                    (Ar)	423.46 m/s
Carbon dioxide    (CO2)	403.25 m/s.

Kinetic energy is the energy that a moving body has. Kinetic energy is defined as the work that must be performed by the force it exerts on the resting body to accelerate it:

Nitrogen:

M= 0.028kg/mol

V²= 505.50m/s²

Ec= ½ 0.028kg/ mol(*505.50m/s) ²

Ec=3577.42 J

The kinetic energy (E) of a body with mass m = 0.028 kilograms and velocity v = 505.50 m/s equals 3577.42 J

Oxygen

M= 0.032kg/mol

V²= 472.85m/s²

Ec= ½ 0.032kg/ mol*(472.85 m/s) ²

Ec= 3577.39 J

The kinetic energy (E) of a body with mass m = 0.032 kilograms and velocity v = 472.85 m/s equals 3577.39 J

Argón

M= 0.0399kg/mol

V²= 423.46m/s

Ec= ½ 0.0399kg/ mol*(423.46 m/s) ²

Ec=3589.92 J

The kinetic energy (E) of a body with mass m = 0.0399 kilograms and velocity v = 423.46 m/s equals 3577.4 J

Carbón Dioxide   

M= 0.044kg/mol

V²= 403.25m/s

Ec= ½ 0.044kg/ mol*(403.25 m/s) ²

Ec= 3577.43 J

The kinetic energy (E) of a body with mass m = 0.044 kilograms and velocity v = 403.25 m/s equals 3577.43 J

 

Kinetic energy of each mole of the different gases

GAS	kinetic energy (Heat)  at 14°C
Nitrogen                  (N2)	3577.42 J
Oxygen                  (O2)	3577.39 J
Argón                     (Ar)	3577.40 J
Carbón Dioxide    (CO2)	3577.43 J.

 

The parts per million of the following gases in the atmosphere
GAS	parts per million
Nitrogen                 (N2)	780.800
Oxygen                    (O2)	209.450
Argón                      (Ar)	9.340
Carbón Dioxide    (CO2)	410

 

 

GAS	VOLUME     PPM	Kinetic energy per Mole gas 14°C	TOTAL(Ek) Mole Gas x Volume 14°C
Nitrogen              (N2)	780.800	3577.42J	2.793.249.536 J
Oxygen               (O2)	209.450	3577.39J	749.284.335 J
Argón                  (Ar)	9.340	3577.40J	33.412.916 J
carbón  Dioxide(CO2)	410	3577.43J	1.466.746 J
TOTAL	1.000.000	3577,41 j	3.577.410.000 J

 

“If you can measure what you are talking about, and if you can express it by a number, then you may think you know something; but if you can't measure it, your knowledge will be poor and unsatisfactory”

Lord Kelvin

Conclusión,

 

GAS	Vcm. Speed Of molecules  at 14°C	Kinetic energy per Mole gas at 14°C	Vcm. Speed Of molecules  at 15°C	Kinetic energy per Mole gas at 15°C
Nitrogen              (N2)	505.50 m/s	3577.42 J	506.38 m/s	3589.89 J
Oxygen               (O2)	472.85 m/s	3577.39 J	473.67 m/s	3589.81 J
Argón                  (Ar)	423.46 m/s	3577.40 J	424.20 m/s	3589.92 J
carbón  Dioxide(CO2)	403.25 m/s.	3577.43 J	403.95 m/s.	3589.86 J.
Average	451.26 m/s	3577,41 J	452.05 m/s	3589.87J

 

The average kinetic energy that originates each gas mole of the 4 main gases in the atmosphere at 15 ° C is 3589.87 J and the molecules move to an average of 452.05 m/s. The gas mole at 14°C, produce a kinetic energy of 3577.41 J, and the molecules move with an average of 451.26 m/s, this leads us to the conclusion that the temperature in the atmosphere increases when the kinetic energy of the molecules in the atmosphere increases, and this increase in the kinetic energy of the molecules, this is due to an increase in the quadratic speed at which molecules move in the atmosphere, According to the data the atmosphere when it goes from 14°C to 15°C, its average kinetic energy increases by 12.46J, and the average velocity of all molecules increases by 1.24m/s, knowing that the atmosphere is made up of 1,000,000 parts of different gases,then the total kinetic energy in the atmosphere would increase by 12.460.000J, which is equivalent to 0.34% of the total kinetic energy.

Finally we can conclude that the kinetic energy by which we can measure the temperature in the atmosphere is governed by the mass of its gas molecules, and the speed at which this mass (molecules) moves, contrary to the explanation of the greenhouse effect, this explains the temperature as a consequence of an infrared absorption and retention phenomenon, by 0.04% of the mass of the gas molecules that make up the atmosphere.

Bibliography

1- Intergovernmental Panel on Climate Change. Consultado el 15 de octubre de 2010.

 A concise description of the greenhouse effect is given in the Intergovernmental Panel on Climate Change Fourth Assessment Report, "What is the Greenhouse Effect?" FAQ 1.3 - AR4 WGI Chapter 1: Historical Overview of Climate Change Science, IIPCC Fourth Assessment Report, Chapter 1, page

2- Maxwell, J. C. (1867). "On the Dynamical Theory of Gases". Philosophical Transactions of the Royal Society of London 157: 49

3-http://www.educaplus.org/gases/ley_charles.html

4-https://www.khanacademy.org/science/chemistry/thermodynamics-chemistry/internal-energy-sal/a/heat

5-https://www.khanacademy.org/science/chemistry/thermodynamics-chemistry/internal-energy-sal/a/heat

6- http://hyperphysics.phy-astr.gsu.edu/hbase/Kinetic/eqpar.html

7- https://en.wikipedia.org/wiki/Equipartition_theorem

8-https://es.wikipedia.org/wiki/Mol#cite_note-avogadro-constant-4

9-https://es.calcprofi.com/energia-cinetica-formula-calculadora.html