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Current Question (ID: 8635)

Question:

$\text{Using the standard electrode potentials of the redox couples given below, which of the following is the strongest oxidizing agent?}$ $\text{E}^\circ \text{ values : Fe}^{3+}/\text{Fe}^{2+} = +0.77\text{ V}$ $\text{I}_2\text{(s)}/\text{I}^- = +0.54\text{ V}$ $\text{Cu}^{2+}/\text{Cu} = +0.34\text{ V}$ $\text{Ag}^+/\text{Ag} = 0.80\text{ V}$

Options:

1. $\text{Fe}^{3+}$
2. $\text{I}_2\text{(s)}$
3. $\text{Cu}^{2+}$
4. $\text{Ag}^+$

Solution:

$\text{Hint: High reduction potential value strongest is the oxidising agent}$ $\text{The given values are as follows:}$ $\text{E}^\circ \text{ values of}$ $\text{Fe}^{3+}/\text{Fe}^{2+} = +0.77\text{V}$ $\text{I}_2\text{(s)}/\text{I}^- = +0.54\text{V}$ $\text{Cu}^{2+}/\text{Cu} = +0.34\text{V}$ $\text{Ag}^+/\text{Ag} = +0.80\text{V}$ $\text{Since, E}^\circ \text{ of the redox couple Ag}^+/\text{Ag is the most positive, i.e., 0.80 V,}$ $\text{therefore Ag}^+ \text{ is the strongest oxidising agent.}$

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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
}