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Current Question (ID: 8558)

Question:

$\text{The oxidation states of the central atom in the given species are, respectively:}$ $\text{H}_4\text{P}_2\text{O}_7 \text{ and H}_2\text{S}_2\text{O}_7$

Options:

1. $0 \text{ and } +6$
2. $+3 \text{ and } +4$
3. $+4 \text{ and } +2$
4. $+5 \text{ and } +6$

Solution:

$\text{Hint: Maximum oxidation number of sulphur is +6}$ $\text{The oxidation number or state of an atom/ion is the number of electrons an atom/ion that the molecule has either gained or lost compared to the neutral atom.}$ $\text{(1) In H}_4\text{P}_2\text{O}_7$ $\text{Let the oxidation number of P = x}$ $\text{Then, we have; } 4(+1) + 2(x) + 7(-2) = 0$ $\Rightarrow 4 + 2x - 14 = 0$ $\Rightarrow x = +5$ $\text{Hence, the oxidation number of P is +5.}$ $\text{(2) In H}_2\text{S}_2\text{O}_7$ $\text{Let the oxidation number of S is x}$ $\text{Then, we have; } 2(+1) + 2(x) + 7(-2) = 0$ $\Rightarrow 2 + 2x - 14 = 0$ $\Rightarrow x = +6$ $\text{Hence, the oxidation number of S is +6.}$ $\text{Therefore, the oxidation states are +5 for P in H}_4\text{P}_2\text{O}_7 \text{ and +6 for S in H}_2\text{S}_2\text{O}_7\text{.}$

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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
}