Total number of electrons present in `11.2 litre` of `NH_(3)` at `STP` are:

Options

A. `6.02 xx 10^(23)`
B. `3.01 xx 10^(23)`
C. `3.01 xx 10^(24)`
D. `5.1 xx 10^(24)`

Explanation

To find the total number of electrons present in 11.2 liters of ammonia (NH₃) at standard temperature and pressure (STP), we can follow these steps:

### Step 1: Determine the number of moles of NH₃ in 11.2 liters at STP.
At STP, 1 mole of any gas occupies 22.4 liters. Therefore, to find the number of moles in 11.2 liters, we can use the formula:

\[ \text{Number of moles} = \frac{\text{Volume of gas}}{\text{Molar volume at STP}} = \frac{11.2 \, \text{liters}}{22.4 \, \text{liters/mole}} = 0.5 \, \text{moles} \]

### Step 2: Calculate the total number of electrons in one mole of NH₃.
The molecular formula for ammonia (NH₃) indicates that it consists of one nitrogen (N) atom and three hydrogen (H) atoms.

- Nitrogen (N) has 7 electrons.
- Each Hydrogen (H) atom has 1 electron, and since there are 3 hydrogen atoms, they contribute a total of \(3 \times 1 = 3\) electrons.

Thus, the total number of electrons in one molecule of NH₃ is:

\[ \text{Total electrons in NH₃} = \text{Electrons from N} + \text{Electrons from H} = 7 + 3 = 10 \, \text{electrons} \]

### Step 3: Calculate the total number of electrons in 0.5 moles of NH₃.
To find the total number of electrons in 0.5 moles of NH₃, we need to multiply the number of electrons in one mole by the number of moles:

\[ \text{Total electrons} = \text{Number of moles} \times \text{Electrons per mole} \times \text{Avogadro's number} \]

Where Avogadro's number (\(N_A\)) is approximately \(6.022 \times 10^{23}\) particles/mole.

Thus,

\[ \text{Total electrons} = 0.5 \, \text{moles} \times 10 \, \text{electrons/molecule} \times 6.022 \times 10^{23} \, \text{molecules/mole} \]

Calculating this gives:

\[ \text{Total electrons} = 0.5 \times 10 \times 6.022 \times 10^{23} = 3.011 \times 10^{24} \, \text{electrons} \]

### Final Answer:
The total number of electrons present in 11.2 liters of NH₃ at STP is \(3.011 \times 10^{24}\) electrons.

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