`4.4 g 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. `6.022xx10^(23)`
B. `1.2044xx10^(23)`
C. `2 "mole"`
D. `6.023xx10^(24)`

Explanation

To solve the problem, we need to find the total number of molecules present in a container when 4.4 g of CO₂ and 2.24 liters of H₂ are mixed at STP (Standard Temperature and Pressure). Here’s a step-by-step breakdown of the solution:

### Step 1: Calculate the number of moles of CO₂

1. **Find the molar mass of CO₂**:
- Carbon (C) = 12 g/mol
- Oxygen (O) = 16 g/mol
- Molar mass of CO₂ = 12 + (2 × 16) = 12 + 32 = 44 g/mol

2. **Calculate the number of moles of CO₂**:
- Given mass of CO₂ = 4.4 g
- Number of moles = mass / molar mass
- Number of moles of CO₂ = 4.4 g / 44 g/mol = 0.1 moles

### Step 2: Calculate the number of moles of H₂

1. **Use the volume of H₂ at STP**:
- At STP, 1 mole of any gas occupies 22.4 liters.
- Given volume of H₂ = 2.24 liters

2. **Calculate the number of moles of H₂**:
- Number of moles of H₂ = volume / molar volume
- Number of moles of H₂ = 2.24 L / 22.4 L/mol = 0.1 moles

### Step 3: Calculate the total number of moles in the container

1. **Add the moles of CO₂ and H₂**:
- Total moles = moles of CO₂ + moles of H₂
- Total moles = 0.1 + 0.1 = 0.2 moles

### Step 4: Calculate the total number of molecules

1. **Use Avogadro's number**:
- Avogadro's number = \(6.022 \times 10^{23}\) molecules/mol

2. **Calculate the total number of molecules**:
- Total molecules = total moles × Avogadro's number
- Total molecules = 0.2 moles × \(6.022 \times 10^{23}\) molecules/mol
- Total molecules = \(1.2044 \times 10^{23}\) molecules

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

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