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Current Question (ID: 18226)

Question:

$\text{For the reduction of silver ions with copper metal, the standard cell potential was found to be } +0.46 \text{ V at } 25 \degree \text{C. The value of standard Gibbs energy, } \Delta G^\circ \text{ will be:}$ $\text{(F = 96500 C mol}^{-1}\text{)}$

Options:

1. $-89.0 \text{ kJ}$
2. $-89.0 \text{ J}$
3. $-44.5 \text{ kJ}$
4. $-98.0 \text{ kJ}$

Solution:

$\text{HINT: Standard Gibbs energy, } \Delta G^\circ = -nF E^\circ_{\text{cell}}$ $\text{Explanation:}$ $\text{For the cell reaction,}$ $2\text{Ag}^+ + \text{Cu} \rightarrow \text{Cu}^{2+} + 2\text{Ag}$ $E^\circ_{\text{cell}} = +0.46 \text{ V}$ $\Delta G^\circ = -2 \times 96500 \times 0.46$ $= -88780 \text{ J}$ $= -88.7 \text{ kJ} \approx -89.0 \text{ kJ}$

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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
}