Question

A compound contains 38.8% C, 16% H and 45.2% N. The formula of the compound would be

Answer 1

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Answer 2

Answer: The formula of the compound would be $CH_5N$.

Explanation:

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C = 38.8 g

Mass of H = 16 g

Mass of N = 45.2 g

Step 1 : convert given masses into moles.

Moles of C =$\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{38.8g}{12g/mole}=3.23moles$

Moles of H=$\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{16g}{1g/mole}=16moles$

Moles of N =$\frac{\text{ given mass of N}}{\text{ molar mass of N}}= \frac{45.2g}{14g/mole}=3.23moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{3.23}{3.23}=1$

For H=$\frac{16}{3.23}=5$

For N= $\frac{3.23}{3.23}=1$

The ratio of C:H:N= 1: 5: 1

Hence the empirical formula is $CH_5N$.