Import Question JSON

Current Question (ID: 8602)

Question:

$\text{The oxidation number of S in } \text{H}_2\text{S}_2\text{O}_8 \text{ is:}$

Options:

1. $+2$
2. $+4$
3. $+6$
4. $+7$

Solution:

$\text{Step I: Find the oxidation state assuming no peroxide linkage.}$ $\text{In } \text{H}_2\text{S}_2\text{O}_8\text{, hydrogen has an oxidation state of } +1 \text{ and oxygen generally has } -2\text{.}$ $\text{Let the oxidation state of S be } x\text{.}$ $2 \times (+1) + 2x + 8 \times (-2) = 0$ $2 + 2x - 16 = 0$ $2x - 14 = 0$ $2x = 14$ $x = +7$ $\text{Step II: Check for abnormality.}$ $\text{Sulfur (S) is in Group 16, and its maximum oxidation state is generally } +6\text{. Since the calculated oxidation state } (+7) \text{ is greater than its maximum possible oxidation state } (+6)\text{, this indicates the presence of a peroxide linkage.}$ $\text{The formula for the number of peroxide linkages is given by:}$ $\text{Number of peroxide linkages} = \frac{\text{Calculated oxidation number} - \text{Group number of central atom}}{2}$ $\text{Number of peroxide linkages} = \frac{+7 - +6}{2} = \frac{1}{2} = 0.5$ $\text{Since the number of peroxide linkages must be a whole number, we round to the nearest whole number, which is 1. This means there is one peroxide linkage.}$ $\text{The chemical structure of } \text{H}_2\text{S}_2\text{O}_8 \text{ (peroxodisulfuric acid or Marshall's acid) is:}$ $\text{H} - \text{O} - \text{S}(\text{=O})_2 - \text{O} - \text{O} - \text{S}(\text{=O})_2 - \text{O} - \text{H}$ $\text{In this structure, two oxygen atoms are in a peroxide linkage (-O-O-), so their oxidation state is } -1 \text{. The remaining six oxygen atoms are singly bonded to sulfur or hydrogen, and their oxidation state is } -2\text{.}$ $\text{Now, recalculate the oxidation state of S considering the peroxide linkage:}$ $\text{Let the oxidation state of S be } X\text{.}$ $2 \times (\text{O.S. of H}) + 2 \times (\text{O.S. of S}) + 6 \times (\text{O.S. of O, normal}) + 2 \times (\text{O.S. of O, peroxide}) = 0$ $2 \times (+1) + 2X + 6 \times (-2) + 2 \times (-1) = 0$ $2 + 2X - 12 - 2 = 0$ $2X - 12 = 0$ $2X = 12$ $X = +6$ $\text{Thus, the oxidation number of S in } \text{H}_2\text{S}_2\text{O}_8 \text{ is } +6\text{.}$

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
}