Chemical Industry

Question 1

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 1

Fritz Haber

IN 1909

Question 1

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 1

Fritz Haber

IN 1909

Question 1

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 1

Fritz Haber

IN 1909

Question 2

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 2

Fritz Haber

IN 1909

Question 2

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 2

Fritz Haber

IN 1909

Question 2

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 2

Fritz Haber

IN 1909

Question 2

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 2

Fritz Haber

IN 1909

Question 2

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 2

Fritz Haber

IN 1909

Question 3

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 3

Fritz Haber

IN 1909

Question 3

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 3

Fritz Haber

IN 1909

Question 4

Who established the conditions under which nitrogen, N2(g) and
hydrogen, H2(g), would combine to give ammonia?

Answer 4

Fritz Haber

IN 1909

Question 5

the process produces ammonia with yiel of approximately _______%

Answer 5

10-20

Question 6

The Haber synthesis was developed into an industrial process by ______________

Answer 6

Carl Bosch

Question 7

is the Haber synthesis endothermic or exothermic? How much energy does it gain/release?

Answer 7

It is an exothermc reaction releasing 92.4 kj/mol

Question 8

Choose the right one

Increasing the pressure causes the equilibrium to move in the forward/reverse direction

Answer 8

Forward

If we increase the pressure, we get more yield

Question 9

Choose the right one

Increasng the temperature causes the equililbrium to move in the forward/reverse direction.

Answer 9

reverse

Decreasing temp causes to move in the forward direction

Question 10

What is the catalyst for the haber process?

Answer 10

Iron

Question 11

Fill the blanks

By using a pressure of around _______ atm and a temperature of about ________ degree celcius, the yield of ammonia is 10-20%

Answer 11

200 and 500

Question 12

True or False

During the industrial production of ammonia, the reaction never reaches equilibrium

Answer 12

True

the gas mixture leaving the reactor is cooled to remove the ammonia

Question 13

what is done with the heat released by the reaction?

Answer 13

It is removed and use to heat the incoming gas mixture

Question 14

What happens to the remaining mixture of reactant gases?

Answer 14

they get recycled throught the reactor

Question 15

what is the process to make sulphuric acid?

Answer 15

Contact Process

Question 16

The manufacture of sulphuric acid by contact process involves the catalytic oxidation
of ________ to _________,

Answer 16

SO2 to SO3

Question 17

Write the steps of the contact process

Answer 17

(i) Solid sulphur, S(s), is burned in air to form sulphric dioxide gas, SO2;
(ii) The gases are mixed with more air then cleaned by electrostatic precipitation
(iii) The mixture of sulphur dioxide and air is heated to 450 °C and subjected to
a pressure of 101.3 - 202.6 kPa (1-2 atmospheres) in the presence of a
vanadium catalyst (vanadium (V) oxide) to produce sulphur trioxide, SO3
(iv) Any unreacted gases from the above reaction are recylced back into the
above reaction.
(v) Sulphur trioxide, SO3(g) is dissolved in 98 % (18 M) sulphuric acid, H2SO4,
to produce disulphuric acid or pyrosulpuric acid, also known as fuming
sulphuric acid or oleum, H2S2O7
very slow.
(vi) Water is added to the disulphuric acid, H2S2O7, to produce sulphuric acid,
H2SO4.
H2S2O7(l) + H2O(l) —→ 2H2SO4(l

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