Goyal Brothers Class-10 Ammonia and Nitric Acid ICSE Chemistry Solutions Ch-9. Step by Step Solutions of Exercise-1 and Exercise -2 , Objective Type Questions of Goyal Brothers Prakashan Chapter-9 Ammonia and Nitric Acid for ICSE Class 10 .

Ammonia and Nitric Acid –  test , use, observation seen , preparation , properties (physical and chemical) of Ammonia and Nitric Acid explain with suitable chemical reaction. Visit official Website CISCE  for detail information about ICSE Board Class-10 Chemistry .

## Goyal Brothers Class-10 Ammonia and Nitric Acid ICSE Chemistry Solutions Ch-9

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Exercise 1

Exercise 2

Objective Type Questions (update soon)

Exercise 1 Page -161

### Goyal Brothers Class-10 Ammonia and Nitric Acid ICSE Chemistry Solutions Ch-9

Question 1.  Complete the following chemical equations and balance them.
(i) (NH4)2 SO4 + NaOH ————>

(ii) (NH4)3 PO4   + KOH    ———–>
(iii) Mg3 N2  +  H2O      ———–>
(iv) AIN     +     H2O      ———->

(i) (NH)4 SO4 + 2NaOH ————> Na2SO4 + 2NH3 + 2H2O

Ammonium Sulfate + Sodium Hydroxide = Sodium Sulfate + Ammonia + Water

(ii) (NH4)3PO4 + 3KOH → K3PO4 + 3NH3 + 3H2O

Tribasic Ammonium Phosphate + Potassium Hydroxide = Tribasic Potassium Phosphate + Ammonia + Water

(iii) Mg3N2 + 6H2O → 3Mg(OH)2 + 2NH3

Magnesium Nitride + Water = Magnesium Hydroxide + Ammonia

(iv) AIN + 3H2O → NH3 + AI(OH)3

Question 2.

(i) How is ammonia gas prepared in the laboratory, starting from NH4CI?
(ii) Name the substance used for drying ammonia gas.
(iii) Why are substances such as conc. H2SO4, anhydrous calcium chloride and phosphorus pentoxide not used for drying ammonia gas?

(i) Preparation in Laboratory

In the laboratory, ammonia is made by heating the ammonium chloride with a quick lime.

2NH4Cl + Ca(OH)2 → CaCl2 + 2H2O + 2NH3

In a rigid glass tube, a mixture of ammonium and quick lime is heated. The received ammonia gas is collected from the gas jar by downward displacement of air.

(ii) drying ammonia gas

the substance used for drying ammonia gas.—Before being collected in a gas jar, ammonia is passed into CaO, which removes the moisture of this gas.

(iii) Concentrated sulphuric acid conc. H2SO4 and anhydrous calcium chloride CaCl2 are not used to dry ammonia because they react with it

Question 3.  By stating experimental conditions, briefly describe Haber’s process for the manufacture of ammonia.

The Haber Process combines nitrogen from the air with hydrogen to form ammonia. The reaction is reversible and the production of ammonia is exothermic.

At each pass of the gases through the reactor, only about 15% of the nitrogen and hydrogen converts to ammonia. Gases are cooled and ammonia turns into liquid. Liquid ammonia is separated and rest of the gas is recycled. By continual recycling of the unreacted nitrogen and hydrogen, we get about 98% of ammonia.

Question 4.  Why is the heating of catalyst discontinued as soon as nitrogen and hydrogen start reacting during Haber’s process?

The electric catalyst in the apparatus is fitted with a heat exchanger
When hydrogen and nitrogen combine ueat is evolved as this reaction is exothermic and therefore the heat exchanger uses this heat to heat the incoming nitrogen and hydrogen gas and external heating is not required

Question 5. Represent Haber’s process by a flowchart.

The optimum conditions are temperature K and Pressure atm.

Question 6. Describe an experiment to show the extreme solubility of ammonia gas in water.

The fountain experiment allows us to prove the extremely high solubility of ammonia in water. . When the syringe is pushed, water enters the inverted flask containing ammonia gas. This gas is highly soluble thus it dissolves almost immediately in it and reduces the pressure in the flask. As the atmospheric pressure outside is more than the pressure inside the flask, it pushes down on the indicator in the beaker and forces it to enter the flask.

This creates a fountain like feature as it enters the flask and changes colour due to ammonia’s basic nature.

Question 7. Write chemical equations when:
(i) Ammonia gas burns in an atmosphere of oxygen.
(ii) Ammonia gas and oxygen in the form of homogeneous mixture is passed over heated platinum.
(iii) Ammonia gas reacts with excess of chlorine gas.
(iv) Ammonia gas reacts with limited amount of chlorine gas.

(i) On burning ammonia in oxygen, the following reaction takes place:

4NH3(g) +3O2(g) 2N2(g) + 6H2O(l)

(ii)

Catalyst used is Platinum. The catalyst glows since the catalytic oxidation of ammonia is an exothermic reaction. The industrial process is known as Ostwald’s process for the manufacture of nitric acid.

## 4NH3(g) +5O2(g) 2N2(g) + 6H2O(l)

(iii)

When the greenish yellow gas chlorine is taken in excess, it reacts with colourless gas ammonia to give a yellow coloured explosive liquid nitrogen trichloride ().

If here ammonia is taken in excess the ammonium chloride is formed.

(iv) Ammonia gas reacts with limited amount of chlorine gas

Produced hydrogen chloride vapor can behave as an acidic compound (can release H+ ions in the water). Then, hydrogen chloride reacts with basic ammonia gas to produce ammonium  chloride which is a solid white smog. To happen this second step reactionammonia is require

Question 8.  Describe an experiment to show the reducing nature of ammonia gas.

Ammonia reduces  to .

Question 9.  Describe all what you will observe and write chemical equations, when a limited amount of ammonia gas is passed through the following aqueous solutions:
(i) ZnCl2 (ii) FeSO4 (iii) FeCl3 (iv) Pb (NO3)2 (v) Cuso4.

when limited amount of ammonia gas is passed through the following aqueous solutions:
(i) ZnCl2

Ammonia gas on reacting with aqueous solution of zinc chloride produces white gelatine like precipitate of zinc hydroxide.

ZnCl2 + 2 NH4OH → Zn (OH)2

(ii) FeSO4

Ammonia gas on reacting with aqueous solution of ferrous sulphate produces dirty green precipitate of ferrous hydroxide.

FeSO4 + 2 NH4OH →(NH4)2SO4 + Fe(OH)2

(iii) FeCl3

(iv) Pb (NO3)2

When ammonia is passed through an aqueous solution of lead nitrate, chalky white precipitate of lead hydroxide is formed which is insoluble in excess of ammonia.

(v) Cuso4.

Question 10.  State four industrial uses of ammonia gas,

Ammonia is also used as a refrigerant gas, for purification of water supplies, and in the manufacture of plastics, explosives, textiles, pesticides, dyes and other chemicals. It is found in many household and industrial-strength cleaning solutions

Question 11. State two tests for ammonia gas.

When added to a solution of copper sulphate, ammonia turns the solution deep blue.

NH3 + CuSO4 + nH2O→ [Cu(NH3)4(H2O)n]SO4

When added to Nessler’s reagent (basic arrangement of K2[HgI4], ammonia gives a precipitate brown in colour.

NH4+ + 2[HgI4]2− + 4OH → HgO·Hg(NH2)I ↓ + 7I + 3H2O

Question 12.  What properties of ammonia gas make it suitable as a refrigerant in cold storages?

It has a low boiling point and is favoured since i) highly energy-efficient refrigerant, having minimal impact on environment ii) having zero Ozone Depletion Potential (ODP) iii) having zero Global Warming Potential (GWP)

Question 13.  What is liquor ammonia? How does it differ from liquid ammonia?

Both liquid and liquor ammonia are in the liquid state. However, the liquid ammonia has only ammonia molecules, but the liquor ammonia has both ammonia and water. The key difference between liquid ammonia and liquor ammonia is that the liquid ammonia contains NH3 molecules, while the liquor ammonia contains NH4OH

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