a compound contains 6.7% hydrogen, 39.9% carbon and rest is oxygen. its molar mass is 60 what are its empirical and molecular formula
Answers
Explanation:
In this question first of all we have to find the percentage of oxygen which can be easily found by simply subtracting percentage of hydrogen & carbon from 100 and then the atomic mass of these elements are taken & the % is divided by their atomic masses & then the least answer is considered & by which all the results are divided & it is rounded off to get integers which gives empirical formula & then the mass of the empirical formula is calculated and is divided by molecular mass which is the value of N & value of N is multiplied to the empirical formula to get answer as acetic acid
The empirical and molecular formula is CH2O and CH3COOH respectively.
Given:
A compound contains 6.7% hydrogen, 39.9% carbon and the rest is oxygen and its molar mass is 60.
To Find:
The empirical and molecular formula.
Solution:
To find the empirical and molecular formula we will follow the following steps:
As we know,
The molecular weight of carbon, oxygen and hydrogen is 12,16 and 1 respectively.
Now,
Oxygen percentage = 100-39.9-6.7 = 53.4
Diving the number of moles with the smallest containing moles we get carbons, oxygen and hydrogen in the empirical formula.
So, the empirical formula = CH2O
The molecular mass of CH2O = 12+2+16 = 30 grams.
Also,
Molecular formula = 2 × empirical formula = 2 × CH2O = C2H4O2 = CH3COOH.
Henceforth, the empirical and molecular formula is CH2O and CH3COOH respectively.