An organic compound containing C,H and N gave the following analysis
C=40 %,H=13.33 %,N=46.67 %
What would be its empirical formula ?

Options

A. `C_(2)H_(7)N`
B. `C_(2)H_(7)N_(2)`
C. `CH_(4)N`
D. `CH_(5)N`

Explanation

To determine the empirical formula of the organic compound containing carbon (C), hydrogen (H), and nitrogen (N) based on the given percentage composition, follow these steps:

### Step 1: Convert the percentages to grams
Assume we have 100 grams of the compound. This means:
- Carbon (C) = 40 g
- Hydrogen (H) = 13.33 g
- Nitrogen (N) = 46.67 g

### Step 2: Convert grams to moles
Using the molar mass of each element:
- Molar mass of C = 12 g/mol
- Molar mass of H = 1 g/mol
- Molar mass of N = 14 g/mol

Calculate the number of moles for each element:
- Moles of C = 40 g / 12 g/mol = 3.33 moles
- Moles of H = 13.33 g / 1 g/mol = 13.33 moles
- Moles of N = 46.67 g / 14 g/mol = 3.33 moles

### Step 3: Divide by the smallest number of moles
Identify the smallest number of moles from the calculations:
- The smallest number of moles is 3.33 (for C and N).

Now, divide the number of moles of each element by the smallest number of moles:
- C: 3.33 / 3.33 = 1
- H: 13.33 / 3.33 = 4
- N: 3.33 / 3.33 = 1

### Step 4: Write the empirical formula
From the ratios obtained:
- C: 1
- H: 4
- N: 1

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

### Conclusion
The empirical formula of the compound is **CH₄N**.