This document discusses ammonia, its properties, production, and reactions. It provides information on collecting ammonia through downward displacement of air and drying it with calcium oxide. Key reactions discussed include producing ammonia from ammonium chloride and calcium hydroxide, and the reducing nature of ammonia shown through its reaction with copper oxide. The Haber and Ostwald processes for producing ammonia and nitric acid respectively are summarized.

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KNOW THE CHEMISTRY
BY RAJIV JAIN

2. THOUGHT FOR THE SESSION

3. THOUGHT FOR THE SESSION

4. AMMONIA

6. Ammonia collection method:

9. Ammonia as reducing agent

11. Ostwald process for manufacturing
Nitric acid

12. Nitric Acid preparation

13. Reactions of ammonia with
mineral acids

16. Important reactions in ammonia

18. TEST FOR AMMONIA
Moist red LITMUS blue /
INIDCATOR/ pH test
Pungent smell
Dense white fumes with HCl
It turns colorless nessler’s reagent
to brown

19. Q1. The gas used as reducing agent in
reducing copper oxide to copper.
Ans1. Ammonia
Q2. Write balanced chemical equations:
Lab preparation of ammonia from
ammonium salts.
ANS 2. NH4Cl + Ca(OH)2 
CaCl2 + NH3 + 2H2O

20. (II)Reaction of ammonia with excess
chlorine.
ANS 2(II)
3Cl2 (excess) + NH3 
NCl3 + 3 HCl

21. (III) Reaction of ammonia with
sulphuric acid.
ANS2 (III) 2 NH3 + H2SO4 
(NH4)2SO4
(IV) Action of warm water on
magnesium nitride.
ANS (IV) Mg3N2 + 6 H2O 
3Mg(OH)2 + 2NH3

22. Q3. (i) Ammonium nitrate is not
used in the preparation of
ammonia because
ANS3 (I) It is explosive in nature
(ii) drying agent during the
process.
ANS3 (II) Calcium oxide

23. (iii) How is ammonia gas
collected?
Ans 3(IV) Downward
displacement of air.
(iv) Explain why it is not collected
over water.
ANS3(IV) Because it is highly
soluble in water.

24. Q4. The diagram shows an experimental set up for the lab
preparation of a pungent smelling gas. The gas is alkaline
in nature.
(i) Name the gas collected in the jar.
ANS 4. ammonia
(ii) Write the balanced equation for the above preparation.
Ans 4 (ii) NH4Cl + Ca(OH)2  CaCl2 + NH3 +
2H2O

25. Q4How is the gas being collected?
ANS4(iii). Downward displacement of air.
(iv)Name the drying agent used.
ANS 4(iv). Quick lime
(v) How will you find that the jar is full of gas?
ANS 4 (v) Bring a rod dipped in hydrogen chloride. Dense
white fumes gives white ppt.

26. Q5. Ammonia can be obtained by adding
water to:
(A) Ammonium chloride.
(B) Ammonium nitrate.
(C) Magnesium nitride.
(D) Magnesium nitrate.
ANS5 (d). Magnesium nitride.
Q6. Identify the following
substances: (i) An alkaline gas A,
which gives dense white fumes with
hydrogen chloride.
ANS 6 (i) Ammonia

27. Q7. Copy and complete the
following table relating to
important industrial
processes. Output refers to
the product of the process
not the intermediate steps.

28. Name of
Process
Inputs Catalyst Equation
for
catalyzed
reaction
Output
Haber
Process
Ammonia
+ Air
Platinum Nitric
acid
Contact
Process
Sulphur
dioxide +
oxygen
Vanadium
peñtoxide

29. Name of
Process
Inputs Catalyst Equation
for
catalyzed
reaction
Output
Haber
Process
Hydrogen
+nitrogen
Finely
divided
iron
N2 + 3H2
 2NH3
Ammonia
Ostwald
process
Ammonia
+ Air
Platinum 4NH3+5O
2 4NO+
6H2O
Nitric acid
Contact
Process
Sulphur
dioxide +
oxygen
Vanadium
pentoxide
2SO2 +O2
 SO3
Sulphuric
acid

30. Q8. Write a balanced equation in
which ammonia is oxidised by:
(i) A metal oxide; (reducing agent
property of ammonia)
3CuO + 2NH3 
3 Cu + N2 + 3H2O
(ii) A gas which is not oxygen.
3Cl2 (excess) +8NH3 
6 NH4Cl + N2

31. Q9. (i) Name the substance used for
drying ammonia.
ANS 9. Calcium oxide or lime
(ii) Write an equation to illustrate
the reducing nature of ammonia.
Ans 9(ii) 3CuO + 2NH3  3 Cu
+ N2 + 3H2O
Copper oxide (black) is reduced to
copper (brown color metallic
copper)

32. Q9. With reference to Haber’s process
for the preparation of ammonia,
write the equation and the
conditions required.
ANS. N2 + 3H2  2NH3
T= 450 0C, 200 atm,
finely divided iron
Prmoter: molybdenum

33. Q10. Write the balanced chemical
equation:
(i) A mixture of ammonium
chloride and slaked lime is
heated.
NH4Cl + Ca(OH)2  CaCl2 +
NH3 + 2H2O
(ii) Aluminium nitride and water.
AlN + 3 H2O  Al(OH)3 +
NH3

34. Q11. The following reaction is carried
out:
A: Nitrogen + metal  compound X
B: X + water  ammonia + other
compound.
C: Ammonia + metal oxide  metal +
water + N2
The one metal which can be used in
reaction A is
Ans. Magnesium.

35. Q11b . The following reaction is carried out:
A: Nitrogen + metal  compound X
B: X + water  ammonia + other compound.
C: Ammonia + metal oxide  metal + water +
N2
(a)State the condition for the reaction
Ans red hot / high temperature
(b) write the formula of the compound X.
Heating
Ans Magnesium hydroxide
(c) What property is demonstrated by reaction
C.
Ans. Reducing agent

36. Q12. Write equations for the
following reactions:
(i) Burning of ammonia in
oxygen
Ans. 4NH3 + 3O2  2N2 + 6H2O
(ii) Catalytic oxidation of
ammonia
Ans. 4NH3+5O2 Pt  4NO+ 6H2O

37. Q13.(i) What do you observe when ammonia
reacted with oxygen in absence of catalyst?
Ans. Greenish yellow flame
(ii) Name the catalyst used.
Ans. platinum
(iii) In the reaction, the catalyst glows red
hot. Why ?
Ans. because reaction takes place at high
temperature.
(iv) What is the name of the industrial
process?
Ans. Ostwald process

38. Q14. What do you observe when
ammonia gas is bubbled through red
litmus solution?
Ans14. Red litmus solution changes to
blue.
Q15. Write a balanced chemical
equation when solution of ammonium
chloride and sodium hydroxide are
mixed and heated.
Ans15.
NH4Cl + NaOH  NaCl + H2O + NH3

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