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Current Question (ID: 21137)

Question:

$\text{Initially 2 moles of } \text{NOCl} \text{ taken in 1 L of closed container and it dissociates into NO and Cl}_2 \text{ gas.}$ $\text{The reaction is as follows:}$ $2\text{NOCl}(g) \rightleftharpoons 2\text{NO}(g) + \text{Cl}_2(g)$ $\text{Calculate the equilibrium constant } K_c \text{ given that 0.4 moles of NO is obtained at equilibrium.}$

Options:

1. $142 \times 10^{-4}$
2. $142 \times 10^{-6}$
3. $125 \times 10^{-4}$
4. $130 \times 10^{4}$

Solution:

$\text{Hint: } K_c = \frac{(\text{NO})^2(\text{Cl}_2)}{(\text{NOCl})^2}$ $2\text{NOCl} \rightleftharpoons 2\text{NO} + \text{Cl}_2$ $\text{Initially}$ $2 \text{ mole } \quad 0 \quad 0$ $\text{At equilibrium } (2-0.4) \quad 0.4 \quad 0.2$ $= 1.6$ $K_c = \frac{(0.4)^2(0.2)}{(1.6)^2}$ $= 0.0125$ $= 125 \times 10^{-4}$

Import JSON File

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
}