a compound contains 92.26% carbon and 7.74% hydrogen. if the molar mass of the compound is 26.038 g mol^-1, then what is its empirical and molecular formulae?
Answers
Answer:
answer
Explanation:
A compound contains 92.26% carbon and 7.74% hydrogen. If the molar mass of the compound is 26.038 g mol −1, then what are its empirical and molecular formulae? Therefore, the empirical formula of the compound is CH.
Answer:
Empirical Formula= CH
Molecular Formula= C2H2
Explanation:
Carbon = 92.26%
Hydrogen = 7.74 %
--Assume it is a 100 gram sample--
C: 92.26 g C x 1 mol C/12.01 g C = 7.682 mol C
H: 7.74 g H x 1 mol H/1.01 g H = 7.663 mol H
--Divide by lowest mole value--
C: 7.682 mol/7.663 mol = 1
H: 7.663 mol/ 7.663 mol = 1
Therefore the Empirical Formula is CH
--Determine molar mass of the empirical formula--
(12.01 g/mol x 1) + (1.01 g/mol x 1) = 13.02 g/mol
--Divide that mass by molar mass--
26.038/13.02 = 1.9998 = 2
--Multiply all subscripts of the Empirical Formula by that value--
CH --> C2H2
Therefore the Molecular Formula is C2H2
(Hope this helps! Have a great day)