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SSLC Chemistry Chapter 7 Important Questions Kerala Syllabus
Some Compounds of Industrial Class 10 Important Questions
Question 1.
Liquefied ammonia is known as ………………….
Answer:
Liquid ammonia
Question 2.
The Industrial preparation of Ammonia is known as ………………………….
a) Haber process
b) Contact process
c) Ostwald process
d) Bosch process
Answer:
a) Haber process
Question 3.
In which one of the following reversible reactions, the change in pressure does not influence the equilibrium?
i. N2(g) + 3H2(g) \(\text { ⇌ }\) 2NH3(g)
ii. N2(g) + O2(g) \(\text { ⇌ }\) 2NO (g)
iii. 2NO(g) + O2(g) \(\text { ⇌ }\) 2NO2(g)
Answer:
N2(g) + O2(g) \(\text { ⇌ }\) 2NO (g)
There is no change in the number of moles of reactants and products.
Question 4.
Write the name of the catalyst used in the industrial production of sulphuric acid.
a) Vanadium pentoxide (V2O5)
b) Platinum (Pt)
c) Iron oxide (Fe2O3 )
d) Manganese oxide (MnO2)
Answer:
a) Vanadium pentoxide (V2O5)
Question 5.
Which industrial process is used to manufacture sulphuric acid (H2SO4)?
A. Contact Process
B. Ostwald Process
C. Deacon Process
D. Haber-Bosch Process
Answer:
A. Contact Process
Question 6.
Match the following.
| Set 1 | Set 2 |
| (a) H2C2O4 | (i) Acid salts |
| (b) NaOH | (ii) Tribasic acid |
| (c) H3PO4 | (iii) Alkali |
| (d) NH4Cl | (iv) Dibasic acid |
Choose the correct answer from the options given below.
Answer:
D. (a) – (iv), (b) – (iii), (c) – (ii), (d) – (i)
Question 7.
Statement 1: Nitrogen, Phosphorous and potassium are the three elements that plants need in large quantities. They are called as primary nutrients.
Statement 2: Elements like Iron and manganese are needed by plants only in very small amounts.
Which of the following is correct regarding the above statements?
A. Both statements are correct
B. Both statements are not correct
C. Only statement 1 is correct
D. Only statement 2 is correct
Answer:
A. Both statements are correct
Question 8.
How do the following conditions affect a reversible reaction?
i. More reactants are added.
ii. Products are removed.
Answer:
i. The rate of forward reaction increases
ii. Rate of forward reaction increases
Question 9.
H2(g) + I2(g) \(\text { ⇌ }\) 2HI(g)
a) What is the total number of moles of reactants and products in the above reaction?
b) What is the effect of pressure in this reversible reaction? Explain.
Answer:
a) No. of moles of reactant = 2
No. of moles of product = 2
b) In a reversible reaction, if there is no change in the number of moles of reactants and products in the gaseous state, pressure will have no effect on the chemical equilibrium.
Question 10.
The flow chart of the industrial preparation of sulphuric acid is given. Complete it.
Answer:
(a) SO2 (Sulphur dioxide)
(b) H2S2O7 (Oleum)
Question 11.
A student dissolves ammonium chloride (NH4Cl) in water and finds the solution is acidic. Explain this observation by answering the following questions.
(a) Identify the acid and base that react to form ammonium chloride (NH4Cl).
(b) Which is stronger, the acid or the base?
Answer:
(a)The acid is Hydrochloric acid (HCl) and the base is Ammonium hydroxide (NH4OH).
(b) The acid (hydrochloric acid) is stronger.
Question 12.
Graph of a reversible process,
N2 + 3H2 \(\text { ⇌ }\) 2NH3 + heat is given. Analyze the graph and answer the following questions.
a) Identify the part of the graph that represents the forward reaction
[OA, BA, AC]
b) Identify the part of the graph which represents the equilibrium state
c) From the given statements, select the correct ones regarding chemical equilibrium.
i. Chemical equilibrium is static at the molecular level.
ii. Both reactants and products co-exist.
iii The rates of forward and backward reactions are equal.
iv. Chemical equilibrium is attained in an open system.
Answer:
a) BA
b) AC
c) (ii) Both reactants and products co-exist.
(iii) The rates of forward and backward reactions are equal
Question 13.
N2(g) + 3H2(g) \(\text { ⇌ }\) 2NH3(g) + Heat
How do the following changes influence the amount of the product?
a) Temperature decreases.
b) Pressure increases.
c) Ammonia produced is removed continuously from the system.
Answer:
a) Amount of product increases
b) Amount of product increases
c) Amount of product increases
Question 14.
a) Which of the following chemicals are used to prepare ammonia (NH3) in the laboratory?
[NaCl, Ca (OH)2, CaCl2, NH4Cl]
b) Ammonia gas produced is passed through quick lime. Give a reason.
c) Which product is obtained when ammonia reacts with HCl?
Answer:
a) NH4CI and Ca(OH)2
b) To remove moisture content.
Quick lime is used as a drying agent.
c) NH3 + HCl → NH4Cl
Question 15.
A few drops of cone. H2SO4 are added to blue coloured copper sulphate crystals taken in a watch glass.
a) Write the observation.
b) Which property of sulphuric acid is exhibited here?
Answer:
a) The blue colour of CuSO4 disappears
b) Dehydrating agent
Question 16.
represents an important stage in the Industrial preparation of Sulphuric acid.
a) By what name is the Industrial preparation of Sulphuric acid known as?
b) How do the following changes influence the forward reaction? :
i) More oxygen (O2) is added
ii) Pressure is decreased
Answer:
a) Contact process
b) i) Increases the rate of forward reaction, and more product is formed.
ii) The rate of forward reaction decreases.
Question 17.
A reversible reaction at equilibrium is given.
2NO(g) + O2(g) \(\text { ⇌ }\) 2NO2(g) + Heat
Answer the following:
a) How does an increase in temperature influence the amount of products formed?
b) What change is to be made in pressure to get more product?
c) How does an increase in the concentration of oxygen influence the rate of the forward reaction?
d) What is the function of a catalyst in reversible reactions?
Answer:
a) Amount of product decreases
b) Increase pressure
c) Forward reaction increases
d) Helps to attain equilibrium more quickly
Question 18.
A reversible reaction at equilibrium is given.
2NO(g) + O2(g) \(\text { ⇌ }\) 2NO2(g)+Heat
a) Write the equation of the forward reaction.
b) How do the following changes affect the rate of forward reaction?
i. Adding more oxygen.
ii. Increasing pressure
c) What is the effect of a catalyst in a reversible reaction at equilibrium?
Answer:
a) 2NO(g) + O2(g) → 2NO2(g)
b) i. Increases,
ii. Increases
c) Catalyst does not affect reversible reactions at equilibrium
Question 19.
a) The industrial preparation of sulphuric acid is known as ___________ .
b) Which is the catalyst used in this process?
c) Take some sugar in a watch glass and add a few drops of concentrated sulphuric acid into it. What is your observation? Which chemical property of sulphuric acid is shown here?
d) Why concentrated sulphuric acid is not used as
drying agent in the preparation of Ammonia?
Answer:
a) Contact process
b) Vanadium pentoxide (V2O5)
c) Sugar is converted into a black substance. The dehydrating nature of sulphuric acid is shown here.
d) Concentrated sulphuric acid is not used as a drying agent in the preparation of ammonia because ammonia is basic and can react with concentrated Sulphuric acid, and then it will form ammonium sulphate.
Question 20.
The presence of various types of nutrients and the specific properties of a fertilizer are critical for
successful plant cultivation.
a) What are the three natural nutrients that plants absorb from air and water?
b) Explain the primary difference between primaiy and secondary nutrients.
c) State two essential qualities a fertilizer must have to be truly effective.
d) Why is a fertilizer that decomposes too quickly considered harmful to plants?
Answer:
a) The three natural nutrients plants absorb from air and wafer are carbon (C), hydrogen (H), and oxygen (O).
b) Primary nutrients are those needed by plants in large quantities, specifically nitrogen (N), phosphorus (P), and potassium (K). In contrast, secondary nutrients are required in smaller amounts and include calcium (Ca), magnesium (Mg), and sulphur (S).
c) Two essential qualities a fertilizer must have are:
- It should be soluble in water so that the nutrients can be absorbed by the plants.
- It should be stable and remain in the soil for a long time, providing a sustained release of nutrients.
d) A fertilizer that decomposes too quickly is harmful because it can cause a “fertilizer burn” that damages the plant’s roots. It also leads to nutrient leaching, which pollutes water, and provides only a brief nutrient boost rather than a steady supply necessary for healthy growth.
Question 21.
The chlor-alkali process is a significant industrial method for producing essential chemicals, including sodium hydroxide, through the electrolysis of brine.
a) What are the ions formed when sodium chloride dissolves in water, and what are their respective charges?
b) At which electrode does oxidation occur, and which ion is oxidised?
c) What is the function of the membrane used to separate the two chambers in the membrane cell?
d) List any two uses of sodium hydroxide.
Answer:
a) When sodium chloride dissolves in water, the
ions formed are sodium ions (Na+), which are positively charged, and chloride ions (Cl–), which are negatively charged.
b) Oxidation occurs at the anode, where the chloride ion (Cl–) is oxidised.
c) The membrane separates the two chambers and allows the passage of specific ions only, such as the Na+ ions moving from the left chamber to the right chamber.
d)
- For the preparation of soaps and detergents.
- For the purification of bauxite in the manufacture of aluminium.