Metallurgy — Maharashtra (SSC) Class 10 Science Solutions (Free)

Free step-by-step Maharashtra (SSC) Class 10 Science solutions for "Metallurgy" — important questions with detailed answers, download PDF for board exam preparation.

Metallurgy — Maharashtra (SSC) Class 10 Science Solutions (Free)

Free step-by-step Maharashtra (SSC) Class 10 Science solutions for "Metallurgy" — important questions with detailed answers, download PDF for board exam preparation.

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Metallurgy — Textbook Questions Answered (7)

Q1: Define metallurgy and explain the reactivity series of metals.

Metallurgy is the science of extracting metals from their ores and purifying them. The reactivity series arranges metals in order of decreasing reactivity: K, Na, Ca, Mg, Al, Zn, Fe, Cu, Hg, Ag, Pt, Au. More reactive metals are extracted using electrolysis, while less reactive metals are extracted by heating with carbon or carbon monoxide.

Q2: What is the difference between roasting and calcination in ore processing?

Roasting is the heating of a sulfide ore in the presence of oxygen to convert it to an oxide. For example, 2PbS + 3O2 → 2PbO + 2SO2. Calcination is the heating of a carbonate ore in the absence of air to drive off CO2. For example, CaCO3 → CaO + CO2. Both are concentration and purification steps.

Q3: Explain electrorefining of copper and its industrial importance.

In electrorefining, impure copper is used as the anode and pure copper as the cathode in a solution of copper sulfate. During electrolysis, copper from the anode dissolves and is deposited on the cathode, while impurities either fall to the bottom as anode mud or remain in solution. This produces 99.99% pure copper used in electrical conductors.

Q4: What is corrosion and how does rusting of iron occur? Name two methods of prevention.

Corrosion is the slow degradation of metals by reaction with atmospheric oxygen and moisture. Rusting: 4Fe + 3O2 + 6H2O → 4Fe(OH)3, a reddish-brown hydrated iron(III) oxide. Prevention methods: painting to exclude air and moisture, galvanizing with zinc coating, oiling, and using stainless steel alloys.

Q5: Explain the thermite process for extraction of metals.

The thermite process uses aluminum as a reducing agent to extract metals from their oxides at high temperatures. For example, Fe2O3 + 2Al → 2Fe + Al2O3 + heat (1600°C). This highly exothermic reaction is used to extract metals like Fe, Cr, Mn that cannot be easily reduced by carbon due to their high reactivity.

Q6: What is an alloy? Give examples of brass and bronze and their uses.

An alloy is a mixture of two or more metals, or a metal with a nonmetal. Brass is Cu + Zn used in decorative items, musical instruments, and electrical parts. Bronze is Cu + Sn used in bells, statues, and machinery bearings. Alloys have improved hardness, strength, and corrosion resistance compared to pure metals.

Q7: Define and differentiate between ferrous and nonferrous metals with examples.

Ferrous metals contain iron as the main component and are magnetic. Examples: iron, steel, cast iron. They are strong, hard, and rust easily. Nonferrous metals do not contain iron. Examples: copper, aluminum, zinc, tin. They are lighter, more corrosion resistant, and often more expensive than ferrous metals.

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