Asample of an unknown compound was decomposed and found to be composed of 1.36 mol oxygen, 4.10 mol hydrogen, and 2.05 mol carbon. what is the empirical formula of the unknown compound? hints a sample of an unknown compound was decomposed and found to be composed of 1.36 mol oxygen, 4.10 mol hydrogen, and 2.05 mol carbon. what is the empirical formula of the unknown compound? c3h6o2 c2h4o c1.5h3o c2h3o

We are given the number of moles:

O = 1.36 mol

H = 4.10 mol

C = 2.05 mol

To get the empirical formula, first divide everything by the smallest number of moles = 1.36 mol. So that:

O = 1 mol

H = 3 mol

C = 1.5 mol

Next step is to multiply everything by a number such that all will be a whole number. In this case, multiply by 2 to get a whole number for C, so that:

O = 2 mol

H = 6 mol

C = 3 mol

Therefore the empirical formula of the compound is:

C3H6O2

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

it is a solid

explanation: