Import Question JSON

Current Question (ID: 8349)

Question:

\text{Select the correct option based on statements below:} \textbf{Assertion (A):} \text{Spontaneous process is an irreversible process and may be reversed by some external agency.} \textbf{Reason (R):} \text{A decrease in enthalpy is a contributing factor to spontaneity.} \text{1. Both (A) and (R) are True and (R) is the correct explanation of (A).} \text{2. Both (A) and (R) are True but (R) is not the correct explanation of (A).} \text{3. (A) is True but (R) is False.} \text{4. (A) is False but (R) is True.}

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:

$\text{Hint: For a spontaneous reaction,}$ $\Delta\text{G value is negative}$ $\text{Let's analyze each statement:}$ $\textbf{Assertion (A):}$ $\text{Spontaneous process is an irreversible process and may be reversed by some external agency.}$ $\text{Analysis of (A):}$ $\text{A spontaneous process is indeed irreversible in the thermodynamic sense. It proceeds naturally in one direction without any external influence. However, it can be reversed by applying external work or energy. For example, water flows spontaneously downhill, but it can be pumped uphill with external energy input. Therefore, assertion (A) is true.}$ $\textbf{Reason (R):}$ $\text{A decrease in enthalpy is a contributing factor to spontaneity.}$ $\text{Analysis of (R):}$ $\text{According to the Gibbs free energy equation:}$ $\Delta\text{G} = \Delta\text{H} - \text{T}\Delta\text{S}$ $\text{For a process to be spontaneous, }\Delta\text{G must be negative. This can be achieved in several ways:}$ $\text{1. }\Delta\text{H is negative (exothermic) and }\Delta\text{S is positive (increasing entropy)}$ $\text{2. }\Delta\text{H is negative and large enough to overcome a negative }\Delta\text{S}$ $\text{3. }\Delta\text{H is positive but }\Delta\text{S is positive and large enough at high temperatures}$ $\text{Therefore, a decrease in enthalpy (negative }\Delta\text{H) does contribute to spontaneity, but it is not the only factor. The reason (R) is true.}$ $\text{Relationship between (A) and (R):}$ $\text{While both statements are true, the reason (R) does not explain why spontaneous processes are irreversible or why they can be reversed by external agency. The reason discusses a thermodynamic criterion for spontaneity (negative }\Delta\text{H), but does not address the irreversibility aspect mentioned in the assertion.}$ $\text{Therefore, option 2 is correct: Both (A) and (R) are True but (R) is not the correct explanation of (A).}$

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
}