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Current Question (ID: 7389)

Question:

$\text{The amount of Zinc (atomic weight = 65) necessary to produce 224 mL of } \text{H}_2 \text{ (at STP) by the reaction with dilute sulphuric acid will be:}$

Options:

1. $0.65 \text{ g}$
2. $7.6 \text{ g}$
3. $6.5 \text{ g}$
4. $8.5 \text{ g}$

Solution:

$\text{Hint: Mole concept-based problem derived from the balanced equation}$\n\n$\text{The reaction is as follows:}$\n\n$\text{Zn} + \text{H}_2\text{SO}_4 \rightarrow \text{ZnSO}_4 + \text{H}_2 \text{ (at STP)}$\n\n$\text{From the balanced equation, 1 mole of Zn produces 22.4 L (or 22400 mL) of } \text{H}_2 \text{ at STP}$\n\n$\frac{224}{22400} = 0.01$\n\n$\text{This means we need 0.01 moles of } \text{H}_2$\n\n$\text{According to the balanced equation, 1 mole of Zn produces 1 mole of } \text{H}_2$\n\n$\text{So, 0.01 moles of } \text{H}_2 \text{ requires 0.01 moles of Zn}$\n\n$\text{Weight of 0.01 Mole of Zn} = 65 \times 0.01$\n\n$= 0.65 \text{ g}$

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
}