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Current Question (ID: 7375)

Question:

$\text{Assertion (A):}$ $\text{1 g O}_2 \text{ and 1 g O}_3 \text{ have an equal number of oxygen atoms.}$ $\text{Reason (R):}$ $\text{O}_2 \text{ and O}_3 \text{ have different molar masses.}$

Options:

1. $\text{Both (A) and (R) are True and (R) is the correct explanation of (A).}$
2. $\text{Both (A) and (R) are True but (R) is not the correct explanation of (A).}$
3. $\text{(A) is True but (R) is False.}$
4. $\text{(A) is False but (R) is True.}$

Solution:

$\text{Hint: Oxygen atom atomic mass is 16 g mol}^{-1}\text{.}$ $\text{The molar mass of O}_2 \text{ is 32 g mol}^{-1} \text{ and the molar mass of O}_3 \text{ is 48 g mol}^{-1}\text{.}$ $\text{Calculate the number of atoms in 1 g O}_2 \text{ as follows:}$ $\text{1 mole O}_2 \text{ is 32 g}$ $\text{The formula for calculating the number of oxygen atoms is as follows:}$ $\text{1 g O}_2$ $= \frac{N_A}{\text{molar mass of O}_2} \times \text{Number of oxygen atom in one O}_2 \text{ molecule}$ $= \frac{6.022 \times 10^{23}}{32} \times 2$ $= 3.8 \times 10^{22} \text{ O atoms}$ $\text{Calculate the number of atoms in 1 g O}_3 \text{ as follows:}$ $\text{1 g O}_3$ $= \frac{N_A}{\text{molar mass of O}_3} \times \text{Number of oxygen atom in one O}_3 \text{ molecule}$ $= \frac{6.022 \times 10^{23}}{48} \times 3$ $= 3.8 \times 10^{22} \text{ O atoms}$ $\text{Hence, both 1 g O}_2 \text{ and 1 g O}_3 \text{ have an equal number of oxygen atoms}$ $\text{Thus, both Assertion & Reason are true but the reason is not the correct explanation of the assertion.}$

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
}