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Current Question (ID: 8561)

Question:

$\text{Which of the following reactions does not involve disproportionation process?}$

Options:

1. $\text{Cl}_2 + \text{OH}^- \rightarrow \text{Cl}^- + \text{ClO}_3^- + \text{H}_2\text{O}$
2. $2\text{H}_2\text{O}_2 \rightarrow \text{H}_2\text{O} + \text{O}_2$
3. $2\text{Cu}^+ \rightarrow \text{Cu}^{2+} + \text{Cu}$
4. $(\text{NH}_4)_2\text{Cr}_2\text{O}_7 \rightarrow \text{N}_2 + \text{Cr}_2\text{O}_3 + 4\text{H}_2\text{O}$

Solution:

$\text{Hint: The same element oxidized and reduced in the compound}$ $\text{Disproportionation reactions are those in which one element undergoes oxidation and reduction both simultaneously.}$ $\text{Analysis of each reaction:}$ $\text{Reaction 1: } \text{Cl}_2 + \text{OH}^- \rightarrow \text{Cl}^- + \text{ClO}_3^- + \text{H}_2\text{O}$ $\text{Cl}_2 \text{ is oxidised to ClO}_3^- \text{ and reduced to Cl}^- \text{. This is disproportionation.}$ $\text{Reaction 2: } 2\text{H}_2\text{O}_2 \rightarrow \text{H}_2\text{O} + \text{O}_2$ $\text{The oxygen atom oxidized from -1 to 0, and reduced from -1 to -2. This is disproportionation.}$ $\text{Reaction 3: } 2\text{Cu}^+ \rightarrow \text{Cu}^{2+} + \text{Cu}$ $\text{Cu}^+ \text{ is oxidized from +1 to +2 and reduced from +1 to 0. This is disproportionation.}$ $\text{Reaction 4: } (\text{NH}_4)_2\text{Cr}_2\text{O}_7 \rightarrow \text{N}_2 + \text{Cr}_2\text{O}_3 + 4\text{H}_2\text{O}$ $\text{Two different elements are oxidized and reduced: Cr is reduced from +6 to +3 and nitrogen is oxidized from -3 to 0.}$ $\text{Since different elements undergo redox changes, this is NOT a disproportionation reaction.}$

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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
}