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Current Question (ID: 9109)

Question:

$\text{The strongest factor responsible for reducing action of Li metal in an aqueous solution is :}$

Options:

1. $\text{Sublimation enthalpy .}$
2. $\text{Ionisation enthalpy.}$
3. $\text{Hydration enthalpy .}$
4. $\text{Electron-gain enthalpy.}$

Solution:

$\text{HINT: High hydration energy.}$ $\text{Explanation:}$ $\text{Lithium ion is small in size and has high ionization enthalpy.}$ $\text{On the other hand, because of its small size, it is extensively hydrated and has very high hydration enthalpy. This high hydration enthalpy compensates for the high energy needed to remove electrons.}$ $\text{Thus, Li has a greater tendency to lose electrons in solution than other alkali metals. The large amount of hydration energy makes it the strongest reducing agent in spite of its highest ionisation enthalpy.}$ $\text{Due to the high hydration energy of } \text{Li}^+ \text{ cation, the standard reduction potential of } \text{Li}^+ \text{ is more negative among all alkali metal cations .}$ $\text{Hence, } \text{Li}^+ \text{ acts as a strong reducing agent in water.}$

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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
}