Import Question JSON

Current Question (ID: 17830)

Question:

$\text{The reaction/s involved during the formation of photochemical smog are:}$ $1. \text{NO}_2(g) \rightarrow \text{NO}(g) + \text{O}(g)$ $2. \text{O}(g) + \text{O}_2(g) \rightarrow \text{O}_3(g)$ $3. \text{O}_3(g) + \text{NO}(g) \rightarrow \text{NO}_2(g) + \text{O}_2(g)$ $4. \text{All of the above}$

Options:

1. $1 \ (5\%)$
2. $2 \ (3\%)$
3. $3 \ (5\%)$
4. $4 \ (89\%)$

Solution:

$\text{HINT: Photochemical smog is formed as a result of the reaction of sunlight}$ $\text{with hydrocarbons and nitrogen oxides.}$ $\text{Explanation:}$ $\text{Ozone, nitric oxide, acrolein, formaldehyde, and peroxyacetyl nitrate (PAN)}$ $\text{are common components of photochemical smog.}$ $\text{The formation of photochemical smog can be summarized as follows:}$ $\text{Burning of fossil fuels leads to the emission of hydrocarbons and nitrogen}$ $\text{dioxide in the atmosphere.}$ $\text{High concentrations of these pollutants in air result in their interaction with}$ $\text{sunlight as follows:}$ $\text{NO}_2(g) \rightarrow \text{NO}(g) + \text{O}(g)$ $\text{O}(g) + \text{O}_2(g) \rightarrow \text{O}_3(g)$ $\text{O}_3(g) + \text{NO}(g) \rightarrow \text{NO}_2(g) + \text{O}_2(g)$ $\text{While ozone is toxic in nature, both NO}_2 \text{ and O}_3 \text{ are oxidizing agents. They react}$ $3\text{CH}_4 + 2\text{O}_3 \rightarrow 3\text{CH} = \text{O} + 3\text{H}_2\text{O}$

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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
}