Which of the following does contain the maximum number of gram molecules ?
(i) 10 g of `H_(2)`, (ii) 34 of `NH_(3)`
(iii) 44g of `CO_(2)`, (iv) 100 g of `H_(2)SO_(4)`

Answer

To determine which of the given substances contains the maximum number of gram molecules (or moles), we will calculate the number of moles for each substance using the formula:

\[ \text{Number of moles} = \frac{\text{Given mass (g)}}{\text{Molar mass (g/mol)}} \]

Let's calculate the number of moles for each option:

### Step 1: Calculate moles of \(H_2\)
- Given mass of \(H_2\) = 10 g
- Molar mass of \(H_2\) = 2 g/mol

\[ \text{Moles of } H_2 = \frac{10 \text{ g}}{2 \text{ g/mol}} = 5 \text{ moles} \]

### Step 2: Calculate moles of \(NH_3\)
- Given mass of \(NH_3\) = 34 g
- Molar mass of \(NH_3\) = 17 g/mol

\[ \text{Moles of } NH_3 = \frac{34 \text{ g}}{17 \text{ g/mol}} = 2 \text{ moles} \]

### Step 3: Calculate moles of \(CO_2\)
- Given mass of \(CO_2\) = 44 g
- Molar mass of \(CO_2\) = 44 g/mol

\[ \text{Moles of } CO_2 = \frac{44 \text{ g}}{44 \text{ g/mol}} = 1 \text{ mole} \]

### Step 4: Calculate moles of \(H_2SO_4\)
- Given mass of \(H_2SO_4\) = 100 g
- Molar mass of \(H_2SO_4\) = 98 g/mol

\[ \text{Moles of } H_2SO_4 = \frac{100 \text{ g}}{98 \text{ g/mol}} \approx 1.02 \text{ moles} \]

### Summary of Moles Calculated:
- Moles of \(H_2\) = 5 moles
- Moles of \(NH_3\) = 2 moles
- Moles of \(CO_2\) = 1 mole
- Moles of \(H_2SO_4\) ≈ 1.02 moles

### Conclusion:
The substance that contains the maximum number of gram molecules is \(H_2\) with 5 moles.

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