Import Question JSON

Current Question (ID: 17837)

Question:

$\text{The reaction(s) involved in ozone layer depletion in the stratosphere is/are:}$

Options:

1. $\text{CF}_2\text{Cl}_2 (g) \xrightarrow{\text{UV}} \cdot \text{Cl} (g) + \cdot \text{CF}_2\text{Cl} (g)$
2. $\cdot \text{Cl} (g) + \text{O}_3 (g) \rightarrow \text{ClO} (g) + \text{O}_2 (g)$
3. $\text{ClO} (g) + \text{O} (g) \rightarrow \cdot \text{Cl} (g) + \text{O}_2 (g)$
4. $\text{All of the above}$

Solution:

$\text{HINT: When chlorine and bromine atoms come into contact with ozone in the stratosphere, they destroy ozone molecules.}$ $\text{STEP 1: In the stratosphere, ozone is a product of the action of UV radiations on dioxygen as:}$ $\text{(i) O}_2 (g) \rightarrow 2\cdot \text{O} (g)$ $\text{(ii) O}_2 (g) + \cdot \text{O} (g) \leftrightarrow \text{O}_3 (g)$ $\text{Reaction (ii) indicates the dynamic equilibrium existing between the production and decomposition of ozone molecules.}$ $\text{STEP 2: Once released CFCs mix with atmospheric gases and reach the stratosphere, where they are decomposed by UV radiations.}$ $\text{(iii) CF}_2\text{Cl}_2 (g) \xrightarrow{\text{UV}} \cdot \text{Cl} (g) + \cdot \text{CF}_2\text{Cl}$ $\text{STEP 3: The chlorine-free radicals produced in reaction (iii) reacts with ozone as:}$ $\text{(iv) } \cdot \text{Cl} (g) + \text{O}_3 (g) \rightarrow \text{ClO} (g) + \text{O}_2 (g)$ $\text{STEP 4: The radicals further react with atomic oxygen to produce more chlorine radicals as:}$ $\text{(v) ClO} (g) + \text{O} (g) \rightarrow \cdot \text{Cl} (g) + \text{O}_2 (g)$ $\text{The regeneration of causes a continuous breakdown of ozone present in the stratosphere, damaging the ozone layer.}$

Import JSON File

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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
}