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Current Question (ID: 8570)

Question:

$\text{The oxidation state of two S-atoms in Na}_2\text{S}_2\text{O}_3 \text{ is:}$

Options:

1. $+2 \text{ and } +4$
2. $+3 \text{ and } -2$
3. $+4 \text{ and } -2$
4. $+6 \text{ and } -2$

Solution:

$\text{Step 1: Consider the structure of Na}_2\text{S}_2\text{O}_3$$ $\text{Na}_2\text{S}_2\text{O}_3 \text{ has a structure where there is a coordinate bond between two sulfur atoms.}$ $\text{There is a coordinate bond between two sulphur atoms. The oxidation number of the acceptor S-atom is -2.}$ $\text{Let the oxidation number of other S-atom be x.}$ $\text{Step 2: Apply the oxidation number balance equation}$ $2(+1) + 3 \times (-2) + x + 1(-2) = 0$ $\text{For Na atoms: } 2(+1) = +2$ $\text{For O atoms: } 3 \times (-2) = -6$ $\text{For coordinate S-atom: } 1(-2) = -2$ $\text{Solving: } +2 - 6 + x - 2 = 0$ $x = +6$ $\text{Step 3: Conclusion}$ $\text{Therefore, the two sulphur atoms in Na}_2\text{S}_2\text{O}_3 \text{ have -2 and +6 oxidation numbers.}$

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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
}