Brook haberprocess1

- 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.

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 C

Here 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!

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 C

Here 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



chemical reactions a set of chemical substance completely transfer into another.

Example - A + B C


Chemical reaction

Sorry ONLY reversible chemical reactions have reverse reaction




Example - A + B C


Chemical reactionREVERSE REACTION

Click Here if you can, to see the reverse reaction




Example - A + B C


Chemical reaction

REVERSE REACTION Click Here if you can to see the reverse reaction Press Here if

You give Up!



Example - A + B C


Chemical reaction

REVERSE REACTION Click Here if you can to see the reverse reaction


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 C

Here A and B react to produce C. and C decompose to produce

Reversible Chemical reaction

REVERSE Click Here to see the reverse reaction

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 C

Here A and B react to produce C. and C decompose to produce

Reversible Chemical reaction

Reverse reaction is possible.

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

In the forward reaction , with the help of a catalyst, Nitrogen and hydrogen produce ammonia and the reverse reaction decomposes ammonia in to




N2 + 3H2 2NH3


Nitrogen Hydrogen Ammonia Heat





N2 + 3H2 2NH3







N2 + 3H2 2NH3







N2 + 3H2 2NH3



Definition


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.

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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

Definition


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.

Change in Equilibrium

Effect of


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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 .


Effect of


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Effect of


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Effect of


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Increase in Nitrogen Concentration


Effect of


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Increase in Hydrogen Concentration


Effect of


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Decrease in Ammonia Concentration


Effect of


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The reaction move to the right and more ammonia 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.

Effect of


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Decrease in Nitrogen Concentration


Effect of


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Decrease in Hydrogen concentration


Effect of


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Increase in Ammonia


Effect of


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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.



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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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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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N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}



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N-N (2) 3 x { H-H ( 2 )} 3 x {N-H-H-H}


Brook haberprocess1

Technology

set of chemical substances

screen chemical reaction

chemical reaction sorry

set of substances

reversible chemical

exothermic reaction

reverse reactionpress

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