4.4 g of a gas at STP occupies a volume of 2.24 L. The gas can be:

Answer

To solve the problem, we need to determine the identity of the gas based on the given mass and volume at standard temperature and pressure (STP). Here’s a step-by-step solution:

### Step 1: Understand the conditions at STP
At standard temperature and pressure (STP), one mole of any ideal gas occupies a volume of 22.4 liters.

### Step 2: Calculate the number of moles of the gas
We can calculate the number of moles of the gas using the formula:
\[ \text{Number of moles} = \frac{\text{Volume of gas at STP}}{\text{Volume occupied by 1 mole at STP}} \]
Given that the volume of the gas is 2.24 L, we can substitute the values:
\[ \text{Number of moles} = \frac{2.24 \, \text{L}}{22.4 \, \text{L/mol}} = 0.1 \, \text{moles} \]

### Step 3: Relate the number of moles to mass
We know that the number of moles is also related to mass and molar mass by the formula:
\[ \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} \]
From the previous step, we have 0.1 moles and the mass of the gas is given as 4.4 g. We can rearrange the formula to find the molar mass:
\[ \text{Molar mass} = \frac{\text{Mass}}{\text{Number of moles}} = \frac{4.4 \, \text{g}}{0.1 \, \text{moles}} = 44 \, \text{g/mol} \]

### Step 4: Identify the gas
Now that we have calculated the molar mass of the gas to be 44 g/mol, we can compare this value with known gases. The molar mass of carbon dioxide (CO₂) is also 44 g/mol.

### Conclusion
Thus, the gas that occupies 2.24 L at STP and has a mass of 4.4 g is carbon dioxide (CO₂).

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