`4.48` litre of methane at S.T.P. corresponds to

Options

A. `1*2xx10^(22)` molecules of methane
B. `0*5` mole of methane
C. `3*2` g of methane
D. `0*1` mole of methane

Explanation

To solve the question regarding what 4.48 liters of methane at STP corresponds to, we can follow these steps:

### Step 1: Understand the conditions at STP
At Standard Temperature and Pressure (STP), the molar volume of any ideal gas is 22.4 liters per mole. This means that 1 mole of gas occupies 22.4 liters at STP.

### Step 2: Calculate the number of moles of methane
To find the number of moles of methane (CH₄) in 4.48 liters, we can use the formula:

\[ \text{Number of moles} = \frac{\text{Volume of gas (L)}}{\text{Molar volume (L/mol)}} \]

Substituting the values:

\[ \text{Number of moles} = \frac{4.48 \, \text{L}}{22.4 \, \text{L/mol}} = 0.2 \, \text{moles} \]

### Step 3: Calculate the mass of methane
Next, we can calculate the mass of methane using its molar mass. The molar mass of methane (CH₄) is calculated as follows:

\[ \text{Molar mass of CH₄} = 12 \, \text{g/mol (C)} + 4 \times 1 \, \text{g/mol (H)} = 16 \, \text{g/mol} \]

Now, we can find the mass of 0.2 moles of methane:

\[ \text{Mass} = \text{Number of moles} \times \text{Molar mass} \]

Substituting the values:

\[ \text{Mass} = 0.2 \, \text{moles} \times 16 \, \text{g/mol} = 3.2 \, \text{grams} \]

### Step 4: Calculate the number of molecules of methane
To find the number of molecules, we can use Avogadro's number, which is approximately \(6.022 \times 10^{23}\) molecules per mole:

\[ \text{Number of molecules} = \text{Number of moles} \times \text{Avogadro's number} \]

Substituting the values:

\[ \text{Number of molecules} = 0.2 \, \text{moles} \times 6.022 \times 10^{23} \, \text{molecules/mole} \approx 1.2044 \times 10^{23} \, \text{molecules} \]

### Conclusion
From the calculations, we find that:
- 4.48 liters of methane at STP corresponds to **0.2 moles of methane**.
- The mass of methane is **3.2 grams**.
- The number of molecules is approximately **1.2044 × 10²³ molecules**.

Thus, the correct answer to the question is **3.2 grams of methane**.

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