Haber Process
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Transcript of Haber Process
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Haber Process
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Haber Process - is a most widely used process to produce ammonia.
- It is mainly the reaction of nitrogen from the air with hydrogen from natural gas to produce ammonia.
Reversibility Equilibrium Exit
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Reversibility.
Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most chemical reactions a set of substances completely transfer into
another substances.
Example - A + B CHere there is no left over A or B. Nearly all of the atoms are converted into C.
Chemical reaction
REVERSE REACTION Click Here if you can to see the reverse reaction
Press Here if You give Up!
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Reversibility.
Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most
chemical reactions a set of substance completely transfer into another substances.
Example - A + B CHere there is no left over A or B. Every single atom is converted into C.
Chemical reaction
REVERSE REACTION Click Here if you can, to see the reverse reaction
Press Here if You give Up!
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Reversibility.
Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer into another.
Example - A + B CHere there is no left over A or B. Every single atom is converted into C.
Chemical reaction
Sorry ONLY reversible chemical reactions have reverse reaction
Press Here if You give Up!
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Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer into another.
Reversibility.
Example - A + B CHere there is no left over A or B. Every single atom is converted into C.
Chemical reactionREVERSE REACTION
Click Here if you can, to see the reverse reaction
Press Here if You give Up!
![Page 7: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/7.jpg)
Reversibility.
Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer into another.
Example - A + B CHere there is no left over A or B. Every single atom is converted into C.
Chemical reaction
REVERSE REACTION Click Here if you can to see the reverse reaction Press Here if
You give Up!
![Page 8: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/8.jpg)
Reversibility.
Chemical reaction is the process that leads transformation of one set of chemical substances in two another substances. In most
chemical reactions a set of chemical substance completely transfer into another.
Example - A + B CHere there is no left over A or B. Every single atom is converted into C.
Chemical reaction
REVERSE REACTION Click Here if you can to see the reverse reaction
Press Here if You give Up!
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Reversibility.
In Reversible Chemical reaction the chemical reaction doesn’t go to completion. Instead it involves both forward reaction ( to
produce product) and back reaction ( to produce reactants ).
Example - A + B CHere A and B react to produce C. and C decompose to produce
Reversible Chemical reaction
REVERSE Click Here to see the reverse reaction
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Reversibility.
In Reversible Chemical reaction the chemical reaction doesn’t go to completion. Instead it involves both forward reaction ( to
produce product) and back reaction ( to produce reactants ).
Example - A + B CHere A and B react to produce C. and C decompose to produce
Reversible Chemical reaction
Reverse reaction is possible.
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Reversibility.
During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
In the forward reaction , with the help of a catalyst Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Application in Haber Process
Nitrogen Hydrogen Ammonia
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In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Reversibility.
During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
Application in Haber Process
Nitrogen Hydrogen AmmoniaForward reactionReverse reaction
Heat
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In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Reversibility.
During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
Application in Haber Process
Nitrogen Hydrogen AmmoniaForward reactionReverse reaction
Heat
![Page 14: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/14.jpg)
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Reversibility.
During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
Application in Haber Process
Nitrogen Hydrogen AmmoniaForward reactionReverse reaction
Heat
![Page 15: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/15.jpg)
In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to
Nitrogen and Hydrogen.
Reversibility.
During Haber process Nitrogen and Hydrogen react and form ammonia. This reaction is reversible that it involves both the production
of reactant and product.
N2 + 3H2 2NH3
Application in Haber Process
Nitrogen Hydrogen AmmoniaForward reactionReverse reaction
Heat
![Page 16: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/16.jpg)
Reversibility.
Now You have a good knowledge about Reversible reactions
So check out what Equilibrium state is.
Equilibrium
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Equilibrium.Definition
Nitrogen Hydrogen Ammonia
The state of a reaction in which both the concentration of the reactant and the product stays the same through out the reaction is called Equilibrium
state.
FeOH
When both the forward and the reverse reactions start going at the same rate , the reaction achieve equilibrium state.
For a reaction to enter equilibrium state it needs to take place in a closed
system.
Watch Animation
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Equilibrium.Definition
Nitrogen Hydrogen Ammonia
The state of a reaction in which both the concentration of the reactant and the product stays the same through out the reaction is called Equilibrium
state.
FeOH
When both the forward and the reverse reactions start going at the same rate , the reaction achieve equilibrium state.
For a reaction to enter equilibrium state it needs to take place in a closed
system.
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Change in Equilibrium
Equilibrium.
Factors which affect equilibrium of a reaction.
Concentration Pressure Temperature
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
But what will happen if the concentration of one of the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
But what will happen if the concentration of one of the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
But what will happen if the concentration of one of the substances change ... ?
Use the arrows to control the concentration .
Nitrogen Hydrogen Ammonia
![Page 23: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/23.jpg)
Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Increase in Nitrogen Concentration
Nitrogen Hydrogen Ammonia
SEEEffect
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Increase in Hydrogen Concentration
Nitrogen Hydrogen Ammonia
SEEEffect
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Decrease in Ammonia Concentration
Nitrogen Hydrogen Ammonia
SEEEffect
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Use the arrows to control the concentration .
The reaction move to the right and more ammonia will be produced.
Nitrogen Hydrogen Ammonia
If a system at equilibrium experiences a change, the system will shift its equilibrium to try to compensate for the change. In doing this new equilibrium will be
achieved.
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Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Decrease in Nitrogen Concentration
Nitrogen Hydrogen Ammonia
SEEEffect
![Page 28: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/28.jpg)
Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Decrease in Hydrogen concentration
Nitrogen Hydrogen Ammonia
SEEEffect
![Page 29: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/29.jpg)
Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Once an equilibrium is established , the concentration of the reactant and the product stays the same through out time ...
Use the arrows to control the concentration .
Increase in Ammonia
Nitrogen Hydrogen Ammonia
SEEEffect
![Page 30: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/30.jpg)
Effect of
Equilibrium.
Concentration
Nitrogen Hydrogen AmmoniaFeOH
Use the arrows to control the concentration .
The reaction move to the left and more Hydrogen and Nitrogens will be produced.
If a system at equilibrium experiences a change, the system will shift its equilibrium to try to compensate for the change. In doing this new equilibrium will be
achieved.
Nitrogen Hydrogen Ammonia
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Equilibrium.
Temperature
Nitrogen Hydrogen AmmoniaFeOH
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Equilibrium.
Temperature
Nitrogen Hydrogen AmmoniaFeOH
When the temperature of the reaction decrease , the exothermic reaction will be favoured because it will
produce the heat that was lost.
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Equilibrium.
Temperature
Nitrogen Hydrogen AmmoniaFeOH
When the temperature of the reaction decrease , the exothermic reaction will be favoured because it will
produce the heat that was lost.
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Equilibrium.
Temperature
Nitrogen Hydrogen AmmoniaFeOH
When the temperature of the reaction decrease , the exothermic reaction will be favoured because it will
produce the heat that was lost.
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Equilibrium.
Pressure
Nitrogen Hydrogen AmmoniaFeOH
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Equilibrium.
Pressure
Nitrogen Hydrogen AmmoniaFeOH
When pressure increases , the system will shift so the least number of gas molecules are formed. The more gas molecules there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules
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Equilibrium.
Pressure
Nitrogen Hydrogen AmmoniaFeOH
When pressure increases , the system will shift so the least number of gas molecules are formed. The more gas molecules there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules
![Page 38: Haber Process](https://reader036.fdocuments.us/reader036/viewer/2022062518/56814329550346895daf9974/html5/thumbnails/38.jpg)
Equilibrium.
Pressure
Nitrogen Hydrogen AmmoniaFeOH
When pressure increases , the system will shift so the least number of gas molecules are formed. The more gas molecules there are, the more collisions there are. These collisions and
the presence of gas molecules are what cause the pressure to increase. Also, when pressure decrease, the system will shift so
the highest number of gas molecules are produced.
N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}
2 molecules 3 molecules 3 molecules