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

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!

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!

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!

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!

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!

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!

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

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.

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

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

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

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

Reversibility.

Now You have a good knowledge about Reversible reactions

So check out what Equilibrium state is.

Equilibrium

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.

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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.

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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.

Change in Equilibrium

Equilibrium.

Factors which affect equilibrium of a reaction.

Concentration Pressure Temperature

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

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

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

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

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

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

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.

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

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

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

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

Equilibrium.

Temperature

Nitrogen Hydrogen AmmoniaFeOH

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.

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.

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.

Equilibrium.

Pressure

Nitrogen Hydrogen AmmoniaFeOH

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

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

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