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Current Question (ID: 18241)

Question:

$\text{For the electrolysis of CuSO}_4 \text{ solution the correct option is:}$

Options:

1. $\text{Cathode reaction: Cu}^{2+} + 2e^- \rightarrow \text{Cu using Cu electrode.}$
2. $\text{Anode reaction: Cu} \rightarrow \text{Cu}^+ + e^- \text{ using Cu electrode.}$
3. $\text{Cathode reaction: 2H}^+ + 2e^- \rightarrow \text{H}_2 \text{ using Pt electrode.}$
4. $\text{Anode reaction: Cu} \rightarrow \text{Cu}^{2+} + 2e^- \text{ using Pt electrode.}$

Solution:

$\text{HINT: In electrolysis at anode oxidation reactions occur.}$ $\text{Explanation:}$ $\text{In electrolysis Cu}^{2+} \text{ ions discharge at the cathode (negatively charged) and the following reaction takes place:}$ $\text{Cu}^{2+} (\text{aq}) + 2e^- \rightarrow \text{Cu} (\text{s})$ $\text{Copper metal is deposited on the cathode. At the anode, copper is converted into Cu}^{2+} \text{ ions by the reaction:}$ $\text{Cu(s)} \rightarrow \text{Cu}^{2+} (\text{s}) + 2e^-$

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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
}