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Current Question (ID: 18222)

Question:

$\text{A steady current of } 1.5 \text{ A flows through a copper voltmeter for } 10 \text{ min. If the electrochemical equivalent of copper is } 30 \times 10^{-5} \text{ g C}^{-1}, \text{ the mass of copper deposited on the electrode will be:}$

Options:

1. $0.40 \text{ g}$
2. $0.50 \text{ g}$
3. $0.67 \text{ g}$
4. $0.27 \text{ g}$

Solution:

$\text{HINT: } m = zit$ $\text{STEP 1:}$ $\text{Given, Current through copper Voltmeter } = 1.5 \text{ A}$ $\text{Time for which current flows } = 10 \text{ min}$ $\text{Electrochemical equivalent of copper } = 30 \times 10^{-5} \text{ g C}^{-1}$ $\text{STEP 2:}$ $\text{If an electric current } I \text{ flows through the electrolyte, then } q = It$ $\therefore m = zit$ $\text{Here, } I = 1.5 \text{ A, } t = 10 \text{ min } = 10 \times 60 \text{ s}$ $z = 30 \times 10^{-5} \text{ g C}^{-1}$ $\text{STEP 3:}$ $\text{Hence, mass of copper deposited on the electrode}$ $m = 30 \times 10^{-5} \times 1.5 \times 10 \times 60$ $= 27 \times 10^{-2} = 0.27 \text{ g}$

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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
}