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Current Question (ID: 18230)

Question:

$\text{Adiponitrile is manufactured electrolytically from acrylonitrile. The reaction is as follows:}$ $\text{CH}_2 = \text{CHCN} \rightarrow \text{CN} - (\text{CH}_2)_4 - \text{CN}$ $\text{How many kg of adiponitrile (molecular mass = 108) is produced in 9.65 hr using a current of 3750 A with 80 \% efficiency?}$

Options:

1. $30 \text{ kg}$
2. $58 \text{ kg}$
3. $60 \text{ kg}$
4. $80 \text{ kg}$

Solution:

$\text{HINT: Faraday's first law of electrolysis.}$ $\text{Explanation:}$ $\text{STEP 1:}$ $2\text{CH}_2 = \text{CHCN} + 2\text{H}^+ + 2e^- \rightarrow \text{CN} - (\text{CH}_2)_4 \text{CN}$ $\text{Current efficiency} = 80\%$ $\text{So effective current} = \frac{80}{100} \times 3750 = 3000 \text{A}$ $\text{STEP 2 :}$ $\text{Using Faraday's First law of electrolysis, we know that;}$ $m = E \times I \times t$ $m = \left( \frac{108}{2} \right) \times 10^{-3} \times 3000 \times 9.65 \times 3600$ $m = \frac{108}{96500} \times 3000 \times 9.65 \times 3600 = 58.32 \text{ kg}$

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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
}