Import Question JSON

Current Question (ID: 7335)

Question:

$\text{The following data was obtained when dinitrogen and dioxygen react together to form different compounds:}$ $\begin{array}{|c|c|c|} \hline & \text{Mass of dinitrogen} & \text{Mass of dioxygen} \\ \hline \text{i.} & 14 \text{ g} & 16 \text{ g} \\ \hline \text{ii.} & 14 \text{ g} & 32 \text{ g} \\ \hline \text{iii.} & 28 \text{ g} & 32 \text{ g} \\ \hline \text{iv.} & 28 \text{ g} & 80 \text{ g} \\ \hline \end{array}$ $\text{The law of chemical combination applicable to the above experimental data is:}$

Options:

1. $\text{Law of reciprocal proportions}$
2. $\text{Law of multiple proportions}$
3. $\text{Law of constant composition}$
4. $\text{None of these}$

Solution:

$\text{HINT: Law of multiple proportions.}$ $\text{For the fixed mass of dinitrogen at 28 g, then the masses of dioxygen that will combine with the fixed mass of dinitrogen are 32 g, 64 g, 32 g, and 80 g. The masses of dioxygen bear a whole number ratio of 1:2:2:5.}$ $\text{Hence, the given experimental data obeys the law of multiple proportions.}$ $\text{The law states that if two elements combine to form more than one compound, then the masses of one element that combines with the fixed mass of another element are in the ratio of small whole numbers.}$

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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
}