Question

A compound is 39.97% carbon, 13.41% hydrogen, and 46.62% nitrogen. What is the empirical formula?

CH4N
CH2N
C2H8N2
C2H4N
(the numbers are subscripts)

Answer 1

CH4N

Step-by-step explanation:

Answer 2

Answer:- First choice is correct. Empirical formula is
`CH_4N` .

Solution:- Mass percentages are given for C, H and N for a compound and we are asked to find out it's empirical formula. First of all we calculate the moles of each element on dividing it's percentage by it's atomic mass;

C =
`39.97g((1mol)/(12.01g))` = 3.33

H =
`13.41g((1mol)/(1.01g))` = 13.3

N =
`46.62g((1mol)/(14.01g))` = 3.33

Let's divide the moles of each by the least one of them which is 3.33.

So, C =
`(3.33)/(3.33)` = 1

H =
`(13.3)/(3.33)` = 4

N =
`(3.33)/(3.33)` = 1

Hence, the empirical formula of the compound is
`CH_4N` . First choice is correct.