Import Question JSON

Current Question (ID: 21090)

Question:

$\text{For the reaction, } 2\text{SO}_2(g) + \text{O}_2(g) = 2\text{SO}_3(g), \Delta H = -57.2 \text{ kJ mol}^{-1} \text{ and } K_C = 1.7 \times 10^{16}. \text{ Which of the following statements is incorrect?}$

Options:

1. $\text{The equilibrium will shift in the forward direction as the pressure increases.}$
2. $\text{The addition of inert gas at constant volume will not affect the equilibrium constant.}$
3. $\text{The equilibrium constant is large suggestive of the reaction going to completion and so no catalyst is required.}$
4. $\text{The equilibrium constant decreases as the temperature increases.}$

Solution:

$\text{1. The } \Delta n_g \text{ value is } -\text{ve for the given reaction. Therefore, the increase in pressure will bring reaction in the forward direction.}$ $\text{2. The change in enthalpy is negative, hence, reaction is an exothermic reaction. Therefore increase in temperature will decrease the equilibrium constant.}$ $\text{3. At constant volume, addition of inert gas will be not affect the equilibrium constant. Equilibrium constant only depends on temperature.}$ $\text{4. The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required. Is not a correct statement. Catalyst only change the rate of reaction. Equilibrium constant did not tells about the time in which reaction gets completed. Hence, catalyst can be used to alter the rate of the reaction.}$

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
}