Import Question JSON

Current Question (ID: 20871)

Question:

$\text{The total energy of 1 mol of photons in J/mol having } \lambda = 600 \text{ nm is:}$ $\text{Given: } h = 6.62 \times 10^{-34} \text{ J sec, } c = 3 \times 10^8 \text{ m s}^{-1}$

Options:

1. $2 \times 10^5 \text{ J/mol}$
2. $6.64 \times 10^8 \text{ J/mol}$
3. $1.24 \times 10^4 \text{ J/mol}$
4. $1.24 \times 10^8 \text{ J/mol}$

Solution:

$\text{Hint: } E_T = \frac{N_A h C}{\lambda}$ $E_T = \frac{N_A h C}{\lambda}$ $\text{or } E_T = \frac{6.02 \times 10^{23} \times 6.62 \times 10^{-34} \times 3 \times 10^8}{600 \times 10^{-9}}$ $= 2 \times 10^5 \text{ J/mol}$

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
}