The percentage of C, H and N in an organic compound are 40% , 13.3% and 46.7% respectively then empirical formula is

Options

A. `C_3H_(13)N_3`
B. `CH_2N`
C. `CH_4N`
D. `CH_6N`

Answer

To find the empirical formula of the organic compound with given percentages of Carbon (C), Hydrogen (H), and Nitrogen (N), we will follow these steps:

### Step 1: Convert the percentages to grams
Assuming we have 100 grams of the compound, the masses of each element will be:
- Carbon (C): 40 grams
- Hydrogen (H): 13.3 grams
- Nitrogen (N): 46.7 grams

### Step 2: Convert grams to moles
Using the atomic masses:
- Carbon (C) = 12 g/mol
- Hydrogen (H) = 1 g/mol
- Nitrogen (N) = 14 g/mol

Now, we can calculate the number of moles for each element:
- Moles of C = 40 g / 12 g/mol = 3.33 moles
- Moles of H = 13.3 g / 1 g/mol = 13.3 moles
- Moles of N = 46.7 g / 14 g/mol = 3.33 moles

### Step 3: Determine the simplest mole ratio
Next, we need to divide the number of moles of each element by the smallest number of moles calculated:
- For C: 3.33 / 3.33 = 1
- For H: 13.3 / 3.33 = 4
- For N: 3.33 / 3.33 = 1

### Step 4: Write the empirical formula
From the ratios calculated, we can write the empirical formula:
- C: 1
- H: 4
- N: 1

Thus, the empirical formula is **CH₄N**.

### Final Answer:
The empirical formula of the compound is **CH₄N**.

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