A compound was found to contain nitrogen 28 g and oxygen 80 g. The formula of the compound is (N = 14, O = 16)

Options

A. `NO`
B. `N_(2)O_(3)`
C. `N_(2)O_(5)`
D. `N_(2)O_(4)`

Answer

To determine the formula of the compound containing nitrogen and oxygen, we can follow these steps:

### Step 1: Calculate the number of moles of nitrogen (N)
Given:
- Mass of nitrogen = 28 g
- Atomic mass of nitrogen (N) = 14 g/mol

Using the formula for moles:
\[ \text{Number of moles of N} = \frac{\text{mass}}{\text{molar mass}} = \frac{28 \text{ g}}{14 \text{ g/mol}} = 2 \text{ moles} \]

### Step 2: Calculate the number of moles of oxygen (O)
Given:
- Mass of oxygen = 80 g
- Atomic mass of oxygen (O) = 16 g/mol

Using the formula for moles:
\[ \text{Number of moles of O} = \frac{\text{mass}}{\text{molar mass}} = \frac{80 \text{ g}}{16 \text{ g/mol}} = 5 \text{ moles} \]

### Step 3: Determine the mole ratio of nitrogen to oxygen
The mole ratio of nitrogen to oxygen can be represented as:
\[ \text{Mole ratio of N to O} = \frac{\text{moles of N}}{\text{moles of O}} = \frac{2}{5} \]

### Step 4: Write the empirical formula
From the mole ratio, we can write the empirical formula of the compound. The empirical formula is based on the simplest whole number ratio of the elements:
- For nitrogen (N): 2
- For oxygen (O): 5

Thus, the empirical formula of the compound is:
\[ \text{Empirical formula} = N_2O_5 \]

### Final Answer
The formula of the compound is \( N_2O_5 \).

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