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Current Question (ID: 18689)

Question:
$\text{The chemical formula for tris(ethane-1,2-diamine)iron(II) phosphate is:}$
Options:
  • 1. $[\text{Fe} (\text{CH}_3-\text{CH} (\text{NH}_2)_2)_3] (\text{PO}_4)_3$
  • 2. $[\text{Fe} (\text{H}_2\text{N-CH}_2-\text{CH}_2-\text{NH}_2)_3] (\text{PO}_4)$
  • 3. $[\text{Fe} (\text{H}_2\text{N-CH}_2-\text{CH}_2-\text{NH}_2)_3] (\text{PO}_4)_2$
  • 4. $[\text{Fe} (\text{H}_2\text{N-CH}_2-\text{CH}_2-\text{NH}_2)_3]_3 (\text{PO}_4)_2$
Solution:
$\text{HINT: Tris indicate that compound contains three ethane-1,2-diamine ligands.}$ $\text{Explanation:}$ $\text{Follow IUPAC rules:}$ $1. \text{Ethane-1,2-diamine(en) is neutral ligand with formula } \text{C}_2\text{H}_4(\text{NH}_2)_2. \text{``Tris'' represents three 'en' ligands are present.}$ $2. \text{Oxidation state of Fe is +2 and two phosphate ligands are outside the complex. Phosphate ligands have -3 charge.}$ $\text{Thus, formula of tris(ethane-1,2-diamine)iron(II)phosphate will be}$ $[\text{Fe} (\text{H}_2\text{N-CH}_2-\text{CH}_2-\text{NH}_2)_3]_3 (\text{PO}_4)_2 \text{ to balance the overall charge.}$

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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
}