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Current Question (ID: 8698)

Question:

$\text{The reaction of aqueous KMnO}_4 \text{ with H}_2\text{O}_2 \text{ in acidic condition gives:}$

Options:

1. $\text{Mn}^{4+} \text{ and O}_2$
2. $\text{Mn}^{2+} \text{ and O}_2$
3. $\text{Mn}^{2+} \text{ and O}_3$
4. $\text{Mn}^{4+} \text{ and MnO}_2$

Solution:

$\text{Hint: KMnO}_4 \text{ acts as an oxidising agent.}$ $\text{Explanation:}$ $\text{The reaction of aqueous KMnO}_4 \text{ with H}_2\text{O}_2 \text{ in acidic conditions is as follows:}$ $2\text{KMnO}_4 + 5\text{H}_2\text{O}_2 + 3\text{H}_2\text{SO}_4 \rightarrow \text{K}_2\text{SO}_4 + 2\text{MnSO}_4 + 8\text{H}_2\text{O} + 5\text{O}_2$ $\text{Here, in the acidic medium the oxidation state of Mn is changing from +7 to +2. So it is acting as an oxidising agent in this case.}$ $\text{Thus, option 2 is the correct answer.}$

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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
}