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Current Question (ID: 10678)

Question:

$\text{Which of the following statements is true?}$

Options:

1. $\text{SO}_2 \text{ bleaches by reduction}$
2. $\text{Cl}_2 \text{ bleaches by oxidation}$
3. $\text{O}_3 \text{ bleaches by oxidation}$
4. $\text{All of the above}$ (Correct)

Solution:

$\text{HINT: Ozone bleaches by oxidation.}$ $\text{Explanation:}$ $\text{1. Bleaching by sulphur dioxide is due to the process of reduction in the presence of moisture.}$ $\text{The reaction is as follows:}$ $\text{SO}_2 + 2\text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4 + 2[\text{H}] \text{ (nascent)}$ $\text{The nascent hydrogen liberated in the reaction is responsible for bleaching action. It gets oxidized and become coloured.}$ $\text{Colour material + [H] \rightarrow \text{Colourless air Colour}$ $\text{2. Bleaching by chlorine is due to the process of oxidation in the presence of moisture.}$ $\text{Cl}_2 + \text{H}_2\text{O} \rightarrow 2\text{HCl} + [\text{O}] \text{ (nascent)}$ $\text{Colour material + [O] \rightarrow \text{Colourless}$ $\text{The oxygen liberated in the reaction is responsible for bleaching, the colour bleached by Cl}_2 \text{ is permanent and the original colour cannot be restored on exposure to air.}$ $\text{3. Ozone liberates atoms of nascent oxygen which acts as an oxidising agent.}$ $\text{Hence ozone bleaches by oxidation.}$ $(\text{O}_3 \rightarrow \text{O}_2 + \text{O})\text{, it acts as a powerful oxidising agent.}$

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Upload a JSON file containing LaTeX/MathJax formatted question, options, and solution.

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
}