Import Question JSON

Current Question (ID: 18843)

Question:

$\text{Which of the following statements is false?}$

Options:

1. $\text{Copper liberates hydrogen from acids.}$
2. $\text{In its higher oxidation states, manganese forms stable compounds with oxygen and fluorine.}$
3. $\text{Mn}^{3+}, \text{ and Co}^{3+} \text{ are oxidizing agents in an aqueous solution.}$
4. $\text{Ti}^{2+}, \text{ and Cr}^{2+} \text{ are reducing agents in an aqueous solution.}$

Solution:

$\text{HINT: Cu does not liberate H}_2 \text{ from acids.}$ $\text{Explanation:}$ $\text{1. Copper lies below hydrogen in the electrochemical series and hence does not liberate H}_2, \text{ from acids. Therefore, option (1) is incorrect.}$ $\text{2. Mn shows the highest oxidation state of +7 with oxygen because it can form } p\pi - d\pi \text{ multiple bonds using 2p orbital of oxygen and 3d orbital of Mn.}$ $\text{On the other hand, Mn shows the highest oxidation state of +4 with fluorine because it can form single bond only.}$ $\text{3. The valence shell electronic configuration of Co(III) is } 3d^6 \text{ and that of Mn(III) is } 3d^4.$ $\text{If Co(III) loses one more electron, then it will have a more stable } 3d^5 \text{ configuration and on loss of one electron Mn(III) forms } 3d^3. \text{ Both forms stable configuration after loss of one electron. Thus, } \text{Mn}^{3+} \text{ and Co}^{3+} \text{ are oxidizing agents in aqueous solution.}$ $\text{4. Ti}^{2+} \text{ and Cr}^{2+} \text{ are reducing agents in an aqueous solution. It is because after loss of one electron both form stable } d^3 \text{ and } d^5 \text{ configuration respectively.}$ $\text{So, options (2, 3, 4) are correct.}$

Import JSON File

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
}