Import Question JSON

Current Question (ID: 7346)

Question:

$\text{Regarding significant figures:}$\n\n$\text{Assertion (A): The significant figure for 0.200 is 3, whereas the significant figure for 200 is 1.}$\n\n$\text{Reason (R): Zero at the end or right of a number is significant, provided it is not on the right side of the decimal point.}$

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:

$\text{Hint: Significant figures are all numbers that add to the meaning of the overall value of the number.}$\n\n$\text{0.200 contains 3 while 200 contains only one significant figure because zero at the end or right of a number are significant provided they are on the right side of the decimal point.}$\n\n$\text{Thus, The assertion is true but the reason is false.}$\n\n$\text{Assertion (A): The significant figure for 0.200 is 3, whereas the significant figure for 200 is 1.}$\n\n$\text{This is correct. In 0.200, all three digits (2, 0, 0) are significant because trailing zeros after the decimal point are always significant. In 200, only the 2 is significant because trailing zeros are not significant unless there is a decimal point.}$\n\n$\text{Reason (R): Zero at the end or right of a number is significant, provided it is not on the right side of the decimal point.}$\n\n$\text{This statement is incorrect. The correct rule is: Zeros at the end or right of a number are significant when they are on the right side of the decimal point. For example, in 0.200, the zeros are significant because they are to the right of the decimal point. In 200, the zeros are not significant because there is no decimal point.}$\n\n$\text{Therefore, option 3 is correct: (A) is True but (R) is False.}$

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
}