Statement-I : `44g` of `CO_(2), 28g` of `CO` have same volume at `STP`
Because
Statement-II : Both `CO_(2)` and `CO` are formed by `C` and oxygen.

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 statements given in the question, we will break down the reasoning step by step.

### Step 1: Understand the Molar Masses
- The molar mass of carbon dioxide (CO₂) is calculated as follows:
- Carbon (C) = 12 g/mol
- Oxygen (O) = 16 g/mol
- Therefore, CO₂ = 12 + (2 × 16) = 12 + 32 = 44 g/mol

- The molar mass of carbon monoxide (CO) is:
- Carbon (C) = 12 g/mol
- Oxygen (O) = 16 g/mol
- Therefore, CO = 12 + 16 = 28 g/mol

### Step 2: Calculate the Number of Moles
- Using the formula for moles (n = mass/molar mass), we can calculate the number of moles for each gas.

For CO₂:
- Mass = 44 g
- Molar mass = 44 g/mol
- Number of moles (n) = 44 g / 44 g/mol = 1 mole

For CO:
- Mass = 28 g
- Molar mass = 28 g/mol
- Number of moles (n) = 28 g / 28 g/mol = 1 mole

### Step 3: Compare the Volumes at STP
- At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters.
- Since both CO₂ and CO have 1 mole, they will occupy the same volume at STP.

### Step 4: Analyze Statement-I
- Statement-I claims that 44 g of CO₂ and 28 g of CO have the same volume at STP.
- Based on our calculations, this statement is true because both gases have the same number of moles and thus occupy the same volume at STP.

### Step 5: Analyze Statement-II
- Statement-II states that both CO₂ and CO are formed by carbon and oxygen.
- This statement is also true. CO₂ is formed from carbon and oxygen (C + O₂ → CO₂), and CO is formed from carbon and oxygen (2C + O₂ → 2CO).

### Conclusion
- Both statements are true, but Statement-II does not provide a correct explanation for Statement-I. Therefore, the conclusion is:
- Statement-I is true, Statement-II is true, but Statement-I is not explained correctly by Statement-II.

### Final Answer
Both statements are correct, but Statement-II is not the correct explanation for Statement-I.

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