Import Question JSON

Current Question (ID: 8110)

Question:

$\text{The incorrect order of the force of attraction among the given species is :}$

Options:

1. $\text{HI} > \text{HBr} > \text{Cl}_2$
2. $\text{CCl}_4 > \text{CH}_2\text{Cl}_2 > \text{CH}_3\text{Cl} > \text{CH}_4$
3. $\text{n-Pentane} > \text{iso-Pentane} > \text{neo-Pentane}$
4. $\text{OH}_2 > \text{O}(\text{CH}_3)_2 > \text{OBr}_2$

Solution:

$\text{HINT: Hydrogen bonding is a stronger force of attraction than dipole-dipole interaction. Iodine is having larger size so, so have higher Vander waal force of attraction which gets reflected in their BP, HI is having -35.3 degree celsius or 237.64 K, where as HBr has -66 degree celsius or 207 k, which contradict polarity law.}$ $\text{Explanation:}$ $\text{Step 1:}$ $\text{(1) In HI, and HBr, the force of attraction is dipole-dipole interaction. The HBr is more polar than HI, hence dipole-dipole interaction is more in the case of HBr. But Iodine is having larger size so, so have higher Vander waal force of attraction which gets reflected in their BP, HI is having -35.3 degree celsius or 237.64 K, where as HBr has -66 degree celsius or 207 k, which contradict polarity law. In } \text{Cl}_2\text{, weak van der waals interactions are present. The correct order is } \text{HI} > \text{HBr} > \text{Cl}_2\text{.}$ $\text{(2) The size of Cl is more than H atom. Cl can show more Van der waals interaction than H. As the number of Cl atoms increases in the molecule van der waals interaction is also increased. Hence, the correct order is } \text{CCl}_4 > \text{CH}_2\text{Cl}_2 > \text{CH}_3\text{Cl} > \text{CH}_4\text{.}$ $\text{(3) In the case of alkane, as branching increases the force of attraction between molecules decreases because the surface area of interaction between molecules decreases. Hence, the correct order is n-Pentane} > \text{iso-Pentane} > \text{neo-Pentane.}$ $\text{(4) The correct order of molecular force is } \text{H}_2\text{O} > \text{OBr}_2 > \text{O}(\text{CH}_3)_2\text{. Water show hydrogen bonding hence, it has the highest molecular force. In the case of } \text{OBr}_2 \text{ and } \text{O}(\text{CH}_3)_2\text{, } \text{O}(\text{CH}_3)_2 \text{ has less dipole-dipole interaction than } \text{OBr}_2 \text{ because in } \text{OBr}_2 \text{ oxygen and bromine bond is more polar than O and C.}$

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
}