how 's manufacturing sulphuric acid?

Question

i want answer in chemical rection ?

Answer 1

Sulfuric acid is produced from sulfur, oxygen and water via the contact process.

In the first step, sulfur is burned to produce sulfur dioxide.

(1) S(s) + O2(g) → SO2(g)
This is then oxidised to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst.

(2) 2 SO2 + O2(g) → 2 SO3(g) (in presence of V2O5)
Finally the sulfur trioxide is treated with water (usually as 97-98% H2SO4 containing 2-3% water) to produce 98-99% sulfuric acid.

(3) SO3(g) + H2O(l) → H2SO4(l)
Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Mists are formed instead of a liquid. Alternatively, the SO3 is absorbed into H2SO4 to produce oleum (H2S2O7), which is then diluted to form sulfuric acid.

(3) H2SO4(l) + SO3 → H2S2O7(l)
Oleum is reacted with water to form concentrated H2SO4.

(4) H2S2O7(l) + H2O(l) → 2 H2SO4(l)
In 1993, American production of sulfuric acid amounted to 36.4 million tonnes. World production in 2001 was 165 million tonnes.

Answer 2

STEP 1:
SO(2) + O(2) --------> SO(3)
Catalyst:- Vanadium pentaoxide
Promoter:-K(2)O [ potassium oxide ]
Temperature:-450--500
Pressure:-1-2 atmospheres

STEP 2:
SO(3) + H(2)SO(4)[conc.] -----------> H(2)S(2)O(7)
( oleum)
sulphur trioxide is not directly converted into sulphuric acid as the reaction is highly exothermic and the sulphuric acid formed gets converted into a fog of sulphuric acid which takes a lot of time to settle down.

STEP 3:
H(2)S(2)O(7) + H(2)O -----------> H(2)SO(4)
THIS SULPHURIC ACID OBTAINED IS 98% concentrated AND IT usually IS NOT concentrated FURTHER ...............



Here is your solution to the preparation of SULPHURIC ACID
and the process is known as the CONTACT PROCESS..........

Answer 3

Its not a simple chemical process / reaction .

The method to obtain H2SO4 product depends on needs .

In Batch Process you have to use HNO3 , H2SO4 ( Dilute )
With Copper & Nickel catalysts with help of Plant circuit designed by Schmiidt .

In Continuos Process same is done but with Biazi Reactor !

FYI - Above processes are called Nitration & are the backbone of Chemical Industries of world .

Answer 4

A brief summary of the Contact Process

The Contact Process:

makes sulphur dioxide;

convers the sulphur dioxide into sulphur trioxide (the reversible reaction at the heart of the process);

converts the sulphur trioxide into concentrated sulphuric acid.



Making the sulphur dioxide

This can either be made by burning sulphur in an excess of air:



. . . or by heating sulphide ores like pyrite in an excess of air:



In either case, an excess of air is used so that the sulphur dioxide produced is already mixed with oxygen for the next stage.

Converting the sulphur dioxide into sulphur trioxide

This is a reversible reaction, and the formation of the sulphur trioxide.

The reasons for all these conditions will be explored in detail further down the page.

Converting the sulphur trioxide into sulphuric acid

This can't be done by simply adding water to the sulphur trioxide - the reaction is so uncontrollable that it creates a fog of sulphuric acid. Instead, the sulphur trioxide is first dissolved in concentrated sulphuric acid:



The product is known as fuming sulphuric acid or oleum.

This can then be reacted safely with water to produce concentrated sulphuric acid - twice as much as you originally used to make the fuming sulphuric acid.





Explaining the conditions

The proportions of sulphur dioxide and oxygen

The mixture of sulphur dioxide and oxygen going into the reactor is in equal proportions by volume.

Avogadro's Law says that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. That means that the gases are going into the reactor in the ratio of 1 molecule of sulphur dioxide to 1 of oxygen.

That is an excess of oxygen relative to the proportions demanded by the equation.



According to Le Chatelier's Principle, Increasing the concentration of oxygen in the mixture causes the position of equilibrium to shift towards the right. Since the oxygen comes from the air, this is a very cheap way of increasing the conversion of sulphur dioxide into sulphur trioxide.

Why not use an even higher proportion of oxygen? This is easy to see if you take an extreme case. Suppose you have a million molecules of oxygen to every molecule of sulphur dioxide.

The equilibrium is going to be tipped very strongly towards sulphur trioxide - virtually every molecule of sulphur dioxide will be converted into sulphur trioxide. Great! But you aren't going to produce much sulphur trioxide every day. The vast majority of what you are passing over the catalyst is oxygen which has nothing to react with.

By increasing the proportion of oxygen you can increase the percentage of the sulphur dioxide converted, but at the same time decrease the total amount of sulphur trioxide made each day. The 1 : 1 mixture turns out to give you the best possible overall yield of sulphur trioxide.



The temperature

Equilibrium considerations

You need to shift the position of the equilibrium as far as possible to the right in order to produce the maximum possible amount of sulphur trioxide in the equilibrium mixture.

The forward reaction (the production of sulphur trioxide) is exothermic.



According to Le Chatelier's Principle, this will be favoured if you lower the temperature. The system will respond by moving the position of equilibrium to counteract this - in other words by producing more heat.

In order to get as much sulphur trioxide as possible in the equilibrium mixture, you need as low a temperature as possible. However, 400 - 450°C isn't a low temperature!

Rate considerations

The lower the temperature you use, the slower the reaction becomes. A manufacturer is trying to produce as much sulphur trioxide as possible per day. It makes no sense to try to achieve an equilibrium mixture which contains a very high proportion of sulphur trioxide if it takes several years for the reaction to reach that equilibrium.

You need the gases to reach equilibrium within the very short time that they will be in contact with the catalyst in the reactor.

The compromise

400 - 450°C is a compromise temperature producing a fairly high proportion of sulphur trioxide in the equilibrium mixture, but in a very short time.



The pressure

Equilibrium considerations



Notice that there are 3 molecules on the left-hand side of the equation, but only 2 on the right.

According to Le Chatelier's Principle, if you increase the pressure the system will respond by favouring the reaction which produces fewer molecules. That will cause the pressure to fall again.

In order to get as much sulphur trioxide as possible in the equilibrium mixture, you need as high a pressure as possible. High pressures also increase the rate of the reaction. However, the reaction is done at pressures close to atmospheric pressure!

Economic considerations

Even at these relatively low pressures, there is a 99.5% conversion of sulphur dioxide into sulphur trioxide. The very small improvement that you could achieve by increasing the pressure isn't worth the expense of producing those high pressures.



The catalyst

Equilibrium considerations

The catalyst has no effect whatsoever on the position of the equilibrium. Adding a catalyst doesn't produce any greater percentage of sulphur trioxide in the equilibrium mixture. Its only function is to speed up the reaction.

Rate considerations

In the absence of a catalyst the reaction is so slow that virtually no reaction happens in any sensible time. The catalyst ensures that the reaction is fast enough for a dynamic equilibrium to be set up within the very short time that the gases are actually in the reactor

Answer 5

sulphuric acid is most potent at 38% dilution

little johnny used to drink
but now he drinks no more
for what he thought was H2O
was H2SO4

Answer 6

How exciting!

S + O2 ---> SO2
SO2 + O2 / V2O5 ---->SO3
SO3 + H2O ----> H2SO4

But in manufacturing, the last step is:

SO3 + H2SO4 ---> H2S2O7
H2S2O7 + H2O ---> H2SO4

Answer 7

H2SO4 is prepared by CONTACT PROCESS

Answer 8

S8(s) + 8O2(g) ---> 8SO2(g)
2SO2(g) + O2(g) --catalyst--> 2SO3(g)
SO3 + H2O ----> H2SO4