Import Question JSON

Current Question (ID: 8560)

Question:

$\text{Why does the MnO}_4^{2-} \text{ ion undergo disproportionation in an acidic medium, whereas the MnO}_4^- \text{ ion does not?}$

Options:

1. $\text{Due to manganese being in its highest oxidation state in MnO}_4^{2-}\text{.}$
2. $\text{Due to manganese being in its highest oxidation state in MnO}_4^-\text{.}$
3. $\text{Because the disproportionation reaction of MnO}_4^{2-} \text{ is endothermic.}$
4. $\text{Because the disproportionation reaction of MnO}_4^{2-} \text{ is exothermic.}$

Solution:

$\text{Hint: Concept of disproportionation in redox reactions}$ $\text{Step 1: Analysis of MnO}_4^{2-}$ $\text{In MnO}_4^{2-} \text{ the oxidation number of Mn is +6. It can increase its oxidation number (to +7) or decrease its oxidation number (to +4, +3, +2, 0).}$ $\text{Hence, it undergoes disproportionation reaction in acidic medium.}$ $\text{The disproportionation reaction is:}$ $3\text{MnO}_4^{2-} + 4\text{H}^+ \rightarrow 3\text{MnO}_4^- + \text{MnO}_2 + 2\text{H}_2\text{O}$ $\text{In this reaction: O.N. increases by 1 per atom (oxidation from +6 to +7), O.N. decreases by 2 per atom (reduction from +6 to +4)}$ $\text{Step 2: Analysis of MnO}_4^-$ $\text{In MnO}_4^- \text{, Mn is in its highest oxidation state, i.e., +7. It can only decrease its oxidation number.}$ $\text{Hence, it cannot undergo a disproportionation reaction.}$ $\text{Conclusion: MnO}_4^- \text{ cannot undergo disproportionation because Mn is already at its maximum oxidation state (+7) and can only be reduced, not simultaneously oxidized and reduced.}$

Import JSON File

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
}