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Current Question (ID: 18535)

Question:

$\text{Consider the following metallurgical process:}$ $\text{Sulfide} \xrightarrow{\Delta} \text{oxide} \xrightarrow{\Delta} \text{Impure metal} \rightarrow \text{pure metal}$ $\text{The processes A, B, and C in the above mentioned reaction are, respectively:}$

Options:

1. $\text{Calcination, smelting, and electrolysis}$
2. $\text{Roasting, smelting, and electrolysis}$
3. $\text{Calcination, auto reduction, and bessemerisation}$
4. $\text{Roasting, aluminothermic reduction, electrolysis}$

Solution:

$\text{HINT: Calcination involves thermal decomposition of carbonate ores.}$ $\text{Explanation:}$ $1. \text{Roasting is a process of heating a sulfide ore to a high temperature in the presence of air. It is a step in the processing of certain ores.}$ $\text{More specifically, roasting is often a metallurgical process involving gas–solid reactions at elevated temperatures with the goal of purifying the metal component(s).}$ $2. \text{Smelting is a form of extractive metallurgy to produce a metal from its ore.}$ $\text{Smelting uses heat and a chemical reducing agent to decompose the ore, driving off other elements as gasses or slag and leaving just the metal behind.}$ $\text{The reducing agent is commonly a source of carbon such as coke, charcoal, and coal.}$ $3. \text{Impure metals can be purified by electrolysis. In an electrolytic cell the anode is made from the crude metal needing to be purified, the cathode from the purified metal.}$ $\text{Thus, the complete process will be:}$ $\text{Metal sulphide} \xrightarrow{\text{Processing}} \text{Metal oxide} \xrightarrow{\text{Smelting}} \text{Metal impure} \xrightarrow{\text{Electrolytic purifying}} \text{Pure metal}$

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Expected JSON Format:

{
  "question": "The mass of carbon present in 0.5 mole of $\\mathrm{K}_4[\\mathrm{Fe(CN)}_6]$ is:",
  "options": [
    {
      "id": 1,
      "text": "1.8 g"
    },
    {
      "id": 2,
      "text": "18 g"
    },
    {
      "id": 3,
      "text": "3.6 g"
    },
    {
      "id": 4,
      "text": "36 g"
    }
  ],
  "solution": "\\begin{align}\n&\\text{Hint: Mole concept}\\\\\n&1 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\text{ moles of carbon atom}\\\\\n&0.5 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\times 0.5 \\text{ mol} = 3 \\text{ mol}\\\\\n&1 \\text{ mol of carbon} = 12 \\text{ g}\\\\\n&3 \\text{ mol carbon} = 12 \\times 3 = 36 \\text{ g}\\\\\n&\\text{Hence, 36 g mass of carbon present in 0.5 mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6].\n\\end{align}",
  "correct_answer": 4
}