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Class 10 Chemistry Chapter 19 Test 8 | Nitrogen and Sulphur
Grade 10 Chemistry Chapter 19 Board Model Paper
Prepare for the Punjab Board Class 10 Chemistry Annual Examination 2027 with Chapter 19: Nitrogen and Sulphur – Class Test No. 8. This comprehensive full chapter test includes textbook exercise questions and is designed as a full chapter model paper to help students evaluate their preparation. Based on the new syllabus issued by PECTAA Punjab, this test is part of our Punjab Board 2027 Model Papers and Chemistry Chapter-Wise Test Series. Practice important Chemistry questions, revise key concepts, assess your understanding, and improve your exam performance with this Class 10 Chemistry Chapter 19 test. Explore our chapter-wise tests and model papers for effective preparation for the 2027 board examinations.
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Full Chapter Test
T-8
CHAPTER # 19
Time:15 mint
(Objective Type)
Total Marks: 12
Note:
Four possible answers A, B, C and D to each question are given. The choice which you think is correct, fill
that circle in front of that question with Marker or Pen ink. Cutting or filling two or more circles will result
in zero mark in that question.
1.
The catalyst used in Haber process is:
(a) Copper
(b) Iron
(c) Zinc
(d) Aluminum
2.
Nitrogen boils at:
(a) −183°C
(b) −100°C
(c) −196°C
(d) 0°C
3.
The purpose of purification of SO2 gas is to:
(a) Increase pressure
(b) Remove impurities like arsenic
(c) Increase temperature
(d) Add oxygen
4.
Metal oxides are generally:
(a) Acidic
(b) Neutral
(c) Basic
(d) Organic
5.
The oxide that is neutral in character:
(a) Al2O3
(b) SO2
(c) CO2
(d) NO
6.
Beryllium and aluminium react with steam at:
(a) Room temperature
(b) 100°C
(c) 700°C
(d) 0°C
7.
Ultraviolet radiation helps in the formation of:
(a) Primary pollutants
(b) Secondary pollutants
(c) Water
(d) Soil
8.
The contact process used for the industrial production of H2SO4 is sensitive to the impurities present in SO2 and O2 because the impurities:
(a) affect the capability of the catalyst
(b) affect the purity of H2SO4
(c) do not let SO2 to react with oxygen
(d) decrease the rate of reaction appreciably
9.
Sodium is considered more reactive than magnesium because:
(a) It is more electropositive than magnesium
(b) It reacts with water slowly.
(c) It is present in second group
(d) It is the less metallic
10.
Secondary pollutants present in the atmosphere are:
(a) Oxides of nitrogen
(b) Oxides of Sulphur
(c) Ozone and PAN
(d) Oxides of Carbon
11.
Oxides formed when oxygen reacts with metals:
(a) Acidic
(b) Basic
(c) Both basic and amphoteric
(d) Neutral
12.
Major components of acid rain are:
(a) H2SO4 and HNO3
(b) H2SO3 and HNO2
(c) H2SO4 and HCl
(d) Acetic Acid and HNO3
Here is Subjective Part of Paper.
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Part – I
2.Write short answers to any Five (5) questions:[5×2=10]
(i)Why is ammonia considered an important industrial chemical?
It is used to make fertilizers (urea, ammonium nitrate, ammonium sulphate), nitric acid, explosives, dyes, plastics and as a refrigerant and cleaning agent.
(ii)How is hydrogen produced from methane?
Methane reacts with steam at about 750–800 °C over a nickel catalyst: CH4 + H2O → CO + 3H2. The CO is then reacted with more steam: CO + H2O → CO2 + H2.
(iii)Why is sulphuric acid important in industry?
It is used to make fertilizers, paints, detergents, plastics, fibres, drugs and car batteries, and in petroleum refining, so it is called the king of chemicals.
(iv)What is the function of concentrated sulphuric acid in the drying tower?
Being strongly hygroscopic, it removes moisture from the SO2 and O2 gases before they reach the catalyst chamber, preventing damage and catalyst poisoning.
(v)What is oleum? How it is formed?
Oleum (fuming sulphuric acid, H2S2O7) is formed when SO3 is absorbed in concentrated H2SO4: H2SO4 + SO3 → H2S2O7.
(vi)Why are metal oxides generally basic in nature?
Metals lose electrons to form positive ions, so their oxides contain the oxide ion (O2−), which accepts H+. They react with acids to give salt and water, and soluble ones give alkalis with water.
(vii)What is Neutral oxide? Give examples.
An oxide that is neither acidic nor basic and does not react with water, acids or bases. Examples: CO, NO, N2O.
(viii)What are metals and where are they found in nature?
Metals are elements that lose electrons to form cations; they are shiny, malleable, ductile and good conductors. Most are found in the earth’s crust combined as ores (oxides, sulphides, carbonates); a few, like gold and platinum, occur free.
3.Write short answers to any Five (5) questions:[5×2=10]
(i)Explain the reaction of group 2 metals with dilute acids.
Group 2 metals react with dilute acids to give a salt and hydrogen, e.g. Mg + 2HCl → MgCl2 + H2. The reaction becomes more vigorous down the group (Ca is faster than Mg).
(ii)Explain the reaction of metals with steam.
Moderately reactive metals react with steam to form metal oxide and hydrogen, e.g. Mg + H2O → MgO + H2; 3Fe + 4H2O ⇌ Fe3O4 + 4H2. Very reactive metals react with cold water, while Cu, Ag and Au do not react.
(iii)How do metals react with oxygen?
Metals combine with oxygen to form basic oxides: 4Na + O2 → 2Na2O; 2Mg + O2 → 2MgO. Reactivity decreases down the reactivity series; gold and platinum do not react.
(iv)What products are formed when sodium burns in air?
Sodium oxide is formed: 4Na + O2 → 2Na2O (with excess oxygen, some sodium peroxide, Na2O2, also forms).
(v)Describe the reaction of metals with dilute acids.
Metals above hydrogen in the reactivity series displace hydrogen from dilute acids, forming a salt: Zn + 2HCl → ZnCl2 + H2. K and Na react violently; Cu, Ag and Au do not react.
(vi)What are primary and secondary pollutants?
Primary: released directly into the air (SO2, NO, CO). Secondary: formed in the atmosphere from reactions of primary pollutants (ozone, PAN, acid rain).
(vii)How are secondary pollutants formed in the atmosphere?
In sunlight, NO2 splits: NO2 → NO + O; then O + O2 → O3. Ozone and NO2 react with volatile organic compounds to form PAN.
(viii)Explain how NOx contributes to the formation of sulphuric acid.
NO2 oxidizes SO2 to SO3: SO2 + NO2 → SO3 + NO. NO is re-oxidized by air to NO2, and SO3 dissolves in rain water: SO3 + H2O → H2SO4.
4.Write short answers to any Five (5) questions:[5×2=10]
(i)Why is ammonia gas turned into a liquid after its production?
Ammonia liquefies easily on cooling (b.p. −33 °C) while unreacted N2 and H2 stay gaseous, so liquefying separates it from them; the liquid is also easier to store and transport.
(ii)How SO2 is prepared from FeS2?
Iron pyrites is roasted in excess air: 4FeS2 + 11O2 → 2Fe2O3 + 8SO2.
(iii)What are the harmful effects of oxides of nitrogen on human health?
They irritate the eyes, nose and throat, damage the lungs, cause breathing problems such as asthma and bronchitis, and lower resistance to respiratory infections.
(iv)How is nitrogen obtained from air?
By fractional distillation of liquid air: nitrogen (b.p. −196 °C) boils off first, leaving oxygen (b.p. −183 °C) behind.
(v)Which conditions are used to oxidize SO2 to SO3 ?
Temperature about 450 °C, pressure 1–2 atm and V2O5 as catalyst: 2SO2 + O2 ⇌ 2SO3.
(vi)How do magnesium and calcium differ with each other towards their reactions with water?
Calcium reacts steadily with cold water giving Ca(OH)2 and H2. Magnesium reacts very slowly with cold water and readily only with steam, so calcium is more reactive.
(vii)The burning of fossil fuels in a car engine is responsible for the production of oxides of nitrogen. Explain.
The very high engine temperature makes N2 and O2 of air combine: N2 + O2 → 2NO; then 2NO + O2 → 2NO2.
(viii)The metals present at the top of the reactivity series are regarded as more reactive than those present at the bottom. Comment on this statement.
The statement is correct. Top metals lose electrons very easily, so they react vigorously with oxygen, water and acids; bottom metals lose electrons with difficulty and react weakly or not at all.
Part – II
NOTE:- Attempt any two questions.[9×2=18]
5.(a) Explain the production of ammonia on industrial scale.
Haber process: N2 (from liquid air) and H2 (from methane + steam) are mixed in 1 : 3 ratio, purified, compressed to 200–250 atm and passed over an iron catalyst at about 450 °C: N2 + 3H2 ⇌ 2NH3 (exothermic). The gas mixture is cooled so ammonia liquefies and is removed; unreacted N2 and H2 are recycled.
(b) Describe the contact process for the production of sulphuric acid.
1) Sulphur or pyrites (FeS2) is burnt in air to give SO2. 2) SO2 and O2 are purified and dried (conc. H2SO4 in drying tower). 3) They pass over V2O5 at about 450 °C and 1–2 atm: 2SO2 + O2 ⇌ 2SO3. 4) SO3 is absorbed in conc. H2SO4 to form oleum (H2S2O7). 5) Oleum is diluted with water to give concentrated H2SO4.
6.(a) Explain the formation and properties of acidic and basic oxides.
Acidic oxides: non-metals burn in oxygen, e.g. S + O2 → SO2; they dissolve in water to give acids (SO2 + H2O → H2SO3) and react with bases to give salts. Basic oxides: metals burn in oxygen, e.g. 2Mg + O2 → 2MgO; soluble ones give alkalis (Na2O + H2O → 2NaOH) and all react with acids to give salt and water.
(b) Differentiate between first and second group metals based on their reactivities with oxygen and water.
Group 1 (Li, Na, K) are more reactive: they tarnish quickly in air, burn to form oxides (4Na + O2 → 2Na2O) and react violently with cold water: 2Na + 2H2O → 2NaOH + H2. Group 2 (Mg, Ca) are less reactive: they burn in oxygen only on heating (2Mg + O2 → 2MgO); Ca reacts steadily with cold water while Mg reacts readily only with steam. Reactivity increases down both groups.
7.(a) What is reactivity series of metals. How it is helpful in predicting their chemical reactions?
The reactivity series arranges metals in decreasing order of reactivity: K, Na, Ca, Mg, Al, Zn, Fe, Pb, (H), Cu, Ag, Au. It helps predict which metals react with oxygen, water and dilute acids, and how vigorously; metals above hydrogen displace H2 from acids, and a more reactive metal displaces a less reactive one from its salt solution.
(b) Describe the role of oxides of nitrogen in the formation of PAN and the acid rain.
PAN: NO2 → NO + O in sunlight; O + O2 → O3; ozone and NO2 react with volatile organic compounds to form PAN (photochemical smog). Acid rain: NO2 dissolves in rain water with oxygen: 4NO2 + O2 + 2H2O → 4HNO3; NO2 also oxidizes SO2 to SO3, which forms H2SO4.
