`{:(,"List-I",,"List-II"),("(P)","0.1 mole",(1),"9 g of water"),("(Q)","0.2 mole",(2),"0.1 g atom of iron"),("(R)","0.25 mole",(3),1.5xx10^(23)"molecules of oxygen gas"),("(S)","0.5 mole",(4),"4480 mL of "CO_(2)" at STP"):}`

Options

A. P-1, Q-3, R-2, S-4
B. P-2, Q-4, R-1, S-3
C. P-2, Q-4, R-3, S-1
D. P-3, Q-1, R-4, S-2

Answer

To solve the problem of matching substances in List-I with their corresponding details in List-II, we will calculate the number of moles for each substance in List-II and then match them with the values in List-I.

### Step-by-Step Solution:

1. **Calculate the number of moles for 9 g of water (List-II: 1)**
- Molar mass of water (H₂O) = 18 g/mol.
- Number of moles = Given mass / Molar mass = 9 g / 18 g/mol = 0.5 moles.
- Thus, 9 g of water corresponds to 0.5 moles.

2. **Calculate the number of moles for 0.1 g atom of iron (List-II: 2)**
- 1 mole of iron (Fe) corresponds to 1 g atom (approximately 56 g).
- Therefore, 0.1 g atom of iron corresponds to 0.1 moles.
- Thus, 0.1 g atom of iron corresponds to 0.1 moles.

3. **Calculate the number of moles for 1.5 x 10²³ molecules of oxygen gas (List-II: 3)**
- Using Avogadro's number (6.022 x 10²³ molecules/mole):
- Number of moles = Number of molecules / Avogadro's number = (1.5 x 10²³) / (6.022 x 10²³) = 0.25 moles.
- Thus, 1.5 x 10²³ molecules of oxygen gas corresponds to 0.25 moles.

4. **Calculate the number of moles for 4480 mL of CO₂ at STP (List-II: 4)**
- At STP, 1 mole of gas occupies 22.4 L (or 22400 mL).
- Number of moles = Volume (mL) / Volume of 1 mole (mL) = 4480 mL / 22400 mL/mole = 0.2 moles.
- Thus, 4480 mL of CO₂ corresponds to 0.2 moles.

### Matching the Results:
- From the calculations:
- (P) 0.1 mole matches with (2) 0.1 g atom of iron.
- (Q) 0.2 mole matches with (4) 4480 mL of CO₂ at STP.
- (R) 0.25 mole matches with (3) 1.5 x 10²³ molecules of oxygen gas.
- (S) 0.5 mole matches with (1) 9 g of water.

### Final Matches:
- P → 2
- Q → 4
- R → 3
- S → 1