hydrocarbon contains 92.3 % C ,Its formula mass= 78 what is the empirical formula and molrculer formula for it

Answer 1

Assume 100 g.

92.3 g C / 12.011 g C/mol = 7.68 mol C
7.7 g H / 1.0079 g H/mol = 7.64 mol H

Roughly 1:1, so the empirical formula is CH, which would have a molecular weight of 13. As the MW is 78, the molecular formula is C6H6, which is benzene.

Answer 2

(92.3/100)*78 =72

so there are 72/12=6 C atoms

Other are hydrogens 78-72 =6
so there are 6 atoms hydrogen

Hydrocarbon C6H6 (benzene)

Answer 3

Formula is C6H6 = Benzene.

It is a cyclic aromatic with alernating single and double bonds.
Mol.mass. = 78. Carbon = 72.....72 ÷ 78 = 0.923 = 92.3%
-C=C-C=C-C=C- Cyclic structure can't be drawn here.
There is 1 Hydrogen on each Carbon.

Answer 4

the 1st step is to assume you have 100g of the compound. It basically makes it much less complicated whilst working with percents, and that's in grams considering the fact that we are working with mass. I.) Carbon constitutes eighty 5.seventy one% of your 100g compound, so its mass is eighty 5.71g. you ought to be waiting to verify what proportion moles that comes out to be. II.) Hydrogen is 14.29% of your compound, so its mass is 14.29g. lower back, discover the quantity of moles. you could now verify the empirical formula. that's the smallest complete quantity ratio of the climate on your hydrocarbon. to discover it, divide each and every of your mole quantities with the help of the least quantity of moles you get carry of as an answer from I and II. working example, in case you discovered C = 0.2333 moles and H = 0.4666 moles, you will divide the two with the help of 0.2333 to get C = a million and H = 2. (that's ok in case you get some thing unusual like H = 2.5 at this factor.) Then plug those values into an empirical formula. In our occasion, you get a million for C and a pair of for H, and your empirical formula would be CH2. in case you get a million for C and a pair of.5 for H, then multiply each and every with the help of two, and you gets C2H5. as long as that's the smallest complete quantity ratio, you're good. Calculate the molar mass of this empirical formula. you have been given a formula mass, and this is your probability to apply it. Divide the formula mass with the help of the mass you gained with the help of your empirical formula. that's the quantity you could desire to multiply each and every ingredient on your empirical formula with the help of as a fashion to get the authentic formula. working example, if the mass of the empirical formula got here out to be 35.06, you will have 70.13/35.06 = 2 (approximately). then you definately would multiply the variety of each and every of the climate on your empirical formula with the help of two to get the authentic formula. Whew!