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Current Question (ID: 18371)

Question:

$\text{Match the items in Column I and Column II:}$ $\begin{array}{|c|c|} \hline \text{Column I} & \text{Column II} \\ \hline \text{A. Mathematical expression for the rate of reaction} & \text{1. Rate constant} \\ \text{B. Rate of reaction for zero-order reaction is equal to} & \text{2. Rate law} \\ \text{C. Units of rate constant for zero-order reaction is same as that of} & \text{3. Order of slowest step} \\ \text{D. Order of a complex reaction is determined by} & \text{4. Rate of reaction} \\ \hline \end{array}$

Options:

1. $\text{3 4 1 2}$
2. $\text{1 2 3 4}$
3. $\text{2 1 4 3}$
4. $\text{4 1 3 2}$

Solution:

$\text{HINT: For zero-order reaction unit of rate constant is } \text{mol L}^{-1}\text{s}^{-1}$ $\text{Explanation:}$ $1. \text{Mathematical expression for the rate of reaction is known as rate law.}$ $2. \text{Rate of reaction for the zero-order reaction is equal to rate constant.}$ $r = k [A]^0$ $\therefore \ r = k$ $3. \text{Unit of the rate of reaction is the same as that of the rate of reaction}$ $4. \text{Order of complex reactions is determined by the rate of a reaction, which is the slowest.}$

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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
}