Four one litre flasks are separately filled with the gases `CO_2`, `F_2`, `NH_3` and He at same room temperature and pressure. The ratio of total number of atoms of these gases present in the different flasks would be

Options

A. `1 : 1 : 1 : 1`
B. `1 : 2 : 2 : 3`
C. `3 : 2 : 4 : 1`
D. `2 : 1 : 3 : 2`

Answer

To solve the problem, we need to determine the total number of atoms present in each gas when filled in one-liter flasks at the same temperature and pressure. Let's break down the solution step by step.

### Step 1: Identify the gases and their molecular formulas
The gases in the flasks are:
- Carbon Dioxide (CO₂)
- Fluorine (F₂)
- Ammonia (NH₃)
- Helium (He)

### Step 2: Determine the number of molecules in each flask
According to Avogadro's hypothesis, equal volumes of gases at the same temperature and pressure contain an equal number of molecules. Since each flask is filled with one liter of gas, they all contain the same number of molecules.

### Step 3: Calculate the number of atoms in each gas
Now, we need to find out how many atoms are in one molecule of each gas:
- **CO₂**: Each molecule has 1 carbon atom and 2 oxygen atoms, totaling **3 atoms**.
- **F₂**: Each molecule has 2 fluorine atoms, totaling **2 atoms**.
- **NH₃**: Each molecule has 1 nitrogen atom and 3 hydrogen atoms, totaling **4 atoms**.
- **He**: Each helium atom is a single atom, totaling **1 atom**.

### Step 4: Establish the ratio of total number of atoms
Now we can express the total number of atoms in each flask as a ratio:
- CO₂: 3 atoms
- F₂: 2 atoms
- NH₃: 4 atoms
- He: 1 atom

Thus, the ratio of the total number of atoms in the flasks is:
\[ \text{CO₂ : F₂ : NH₃ : He} = 3 : 2 : 4 : 1 \]

### Final Answer
The ratio of total number of atoms of these gases present in the different flasks is **3 : 2 : 4 : 1**.

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