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Current Question (ID: 17634)

Question:

$\text{Given below is a reaction sequence:}$ $\text{(a)} \quad \text{CH}_3 - \text{CH} - \text{CH} - \text{CH}_3 \xrightarrow{\text{H}^+/\text{Heat}} \text{A} + \text{B}$ $\text{(b)} \quad \text{HBr, dark} \quad \text{in absence of peroxide} \quad \text{C} + \text{D}$ $\text{The compounds A and C are respectively:}$

Options:

1. $\text{CH}_3 \vert \text{CH}_3 - \text{C} = \text{CH}_2 \quad \text{and} \quad \text{CH}_3 - \text{C} - \text{CH}_2 - \text{CH}_3 \vert \text{Br}$
2. $\text{CH}_3 \vert \text{CH}_3 - \text{C} = \text{CH}_2 \quad \text{and} \quad \text{CH}_3 - \text{CH} - \text{CH} - \text{CH}_3 \vert \text{Br}$
3. $\text{CH}_3 \vert \text{CH}_2 = \text{C} - \text{CH}_3 \quad \text{and} \quad \text{CH}_3 - \text{C} - \text{CH}_2 - \text{CH}_3 \vert \text{Br}$
4. $\text{CH}_3 \vert \text{CH}_2 = \text{C} - \text{CH}_3 \quad \text{and} \quad \text{CH}_2 - \text{CH} - \text{CH}_2 - \text{CH}_3 \vert \text{Br}$

Solution:

$\text{Hint: The first reaction is an example of an elimination reaction}$ $\text{Step 1:}$ $\text{The first reaction is an elimination reaction and then an electrophilic addition reaction takes place.}$ $\text{The reaction occurs with the rearrangement of the carbocation.}$ $\text{In the first reaction, alcohol is converted into an alkene. The reaction is as follows:}$ $\text{CH}_3 \vert \text{CH}_3 - \text{CH} - \text{CH}_2 \xrightarrow{\text{H}^+/\Delta} \text{CH}_3 - \text{CH} = \text{CH}_2 \quad \text{minor (B)}$ $\text{Step 2:}$ $\text{In the second step, the major product reacts with HBr and give an electrophilic addition reaction.}$ $\text{In this reaction, an alkene is converted into alkyl bromide.}$ $\text{The reaction is as follows:}$ $\text{CH}_3 \vert \text{CH}_3 - \text{C} = \text{CH}_2 \xrightarrow{\text{HBr (dark)}} \text{CH}_3 - \text{C} - \text{CH}_2 - \text{CH}_3 \vert \text{Br} \quad \text{Major (C)}$

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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
}