`4.4 gm of CO_(2)` and `2.24 "litre" of H_(2)` at `STP` are mixed in a container. The total number of molecules present in the container will be:

Options

A. `9.9`
B. `0.099`
C. `0.001`
D. `1.00`

Explanation

To solve the problem of finding the total number of molecules present in a container with 4.4 g of CO₂ and 2.24 liters of H₂ at STP, we can follow these steps:

### Step 1: Calculate the number of moles of CO₂
- Given mass of CO₂ = 4.4 g
- Molar mass of CO₂ = 44 g/mol

Using the formula for moles:
\[ \text{Number of moles of CO₂} = \frac{\text{Given mass}}{\text{Molar mass}} = \frac{4.4 \text{ g}}{44 \text{ g/mol}} = 0.1 \text{ moles} \]

### Step 2: Calculate the number of moles of H₂
- Given volume of H₂ = 2.24 liters
- At STP, 1 mole of gas occupies 22.4 liters.

Using the formula for moles:
\[ \text{Number of moles of H₂} = \frac{\text{Given volume}}{22.4 \text{ L/mol}} = \frac{2.24 \text{ L}}{22.4 \text{ L/mol}} = 0.1 \text{ moles} \]

### Step 3: Calculate the total number of moles in the container
\[ \text{Total number of moles} = \text{Number of moles of CO₂} + \text{Number of moles of H₂} = 0.1 + 0.1 = 0.2 \text{ moles} \]

### Step 4: Calculate the total number of molecules
Using Avogadro's number (approximately \(6.022 \times 10^{23}\) molecules/mol):
\[ \text{Total number of molecules} = \text{Total number of moles} \times \text{Avogadro's number} = 0.2 \text{ moles} \times 6.022 \times 10^{23} \text{ molecules/mol} \]
\[ = 1.2044 \times 10^{23} \text{ molecules} \]

### Final Answer
The total number of molecules present in the container is approximately \(1.2044 \times 10^{23}\) molecules.

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