Statement-1 : If same amounts are considered `CO_(2)` requires more heat than `O_(2)`, for the same rise in temperature.
And
Statement-2 : `CO_(2)` being triatomic has higher heat capacity than `O_(2)`

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is Not a correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is False
D. Statement-1 is False, Statement-2 is True

Answer

To solve the question, we need to analyze both statements and determine their correctness and whether Statement 2 provides a valid explanation for Statement 1.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- Statement 1 claims that for the same amounts of gas, carbon dioxide (CO₂) requires more heat than oxygen (O₂) for the same rise in temperature.
- We know that the amount of heat required to raise the temperature of a substance is given by the formula:
\[ \Delta H = n C_p \Delta T \]
where:
- \(\Delta H\) = change in enthalpy (heat absorbed)
- \(n\) = number of moles
- \(C_p\) = heat capacity at constant pressure
- \(\Delta T\) = change in temperature

2. **Analyzing the Parameters**:
- Since the question states "if same amounts are considered," we can assume that \(n\) (number of moles) and \(\Delta T\) (change in temperature) are the same for both gases.
- Therefore, the heat required will depend on the \(C_p\) values of CO₂ and O₂.

3. **Comparing Heat Capacities**:
- Carbon dioxide (CO₂) is a triatomic molecule, while oxygen (O₂) is diatomic.
- The heat capacity at constant pressure (\(C_p\)) for different types of gases can be determined from their molecular structure:
- For a linear triatomic gas like CO₂, the \(C_p\) value is:
\[ C_p = \frac{9}{2} R \]
- For a diatomic gas like O₂, the \(C_p\) value is:
\[ C_p = \frac{7}{2} R \]
- Since \(\frac{9}{2} R > \frac{7}{2} R\), it follows that \(C_p\) for CO₂ is greater than that for O₂.

4. **Conclusion for Statement 1**:
- Since CO₂ has a higher heat capacity than O₂, it indeed requires more heat for the same rise in temperature.
- Therefore, Statement 1 is **correct**.

5. **Understanding Statement 2**:
- Statement 2 states that CO₂ being triatomic has a higher heat capacity than O₂.
- This is consistent with our earlier analysis where we found that \(C_p\) for CO₂ is greater than that for O₂.

6. **Conclusion for Statement 2**:
- Statement 2 is also **correct** and correctly explains Statement 1.

### Final Answer:
Both Statement 1 and Statement 2 are true, and Statement 2 is a correct explanation for Statement 1.