Assertion: A molecule of butane, `C_(4)H_(10)` has a mass of `58.12 amu`.
Reason: One mole of butane contains `6.022xx10^(23)` molecules and has a mass of `58.12 g`.

Options

A. Statement-I is true, Statement-II is true , Statement-II is correct explanation for Statement-I
B. Statement-I is true, Statement-II is true , Statement-II is `NOT` a correct explanation for statement-I
C. Statement-I is true, Statement-II is false
D. Statement-I is false, Statement-II is true

Answer

To analyze the assertion and reason provided in the question, we can break down the solution into a few clear steps:

### Step 1: Understand the Assertion
The assertion states that a molecule of butane, \(C_4H_{10}\), has a mass of \(58.12 \, \text{amu}\).

- **Calculation of Molar Mass of Butane**:
- The molar mass of butane can be calculated by adding the atomic masses of its constituent atoms:
- Carbon (C): 12.01 amu (4 atoms)
- Hydrogen (H): 1.008 amu (10 atoms)
- Therefore, the molar mass calculation is:
\[ \text{Molar mass of } C_4H_{10} = (4 \times 12.01) + (10 \times 1.008) = 48.04 + 10.08 = 58.12 \, \text{amu} \]
- This confirms that the assertion is true.

### Step 2: Understand the Reason
The reason states that one mole of butane contains \(6.022 \times 10^{23}\) molecules and has a mass of \(58.12 \, \text{g}\).

- **Understanding Moles**:
- By definition, one mole of any substance contains \(6.022 \times 10^{23}\) entities (Avogadro's number).
- Since the molar mass of butane is \(58.12 \, \text{g/mol}\), one mole of butane indeed has a mass of \(58.12 \, \text{g}\).
- This also confirms that the reason is true.

### Step 3: Conclusion
Both the assertion and reason are true and the reason correctly explains the assertion.

### Final Answer
Both the assertion and the reason are correct, and the reason provides a valid explanation for the assertion.

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