Iam finding the formula of a compound that has 60% carbon, 32% oxygen, and 8% hydrogen. although, when it comes to actually creating the formula i end up with a subscript of 2.5 for c, 1 for o, and 4 for h.
i know i have to double each subscript for the empirical formula, but i am not sure what to do after that in terms of getting the molecular formula.

Explanation:

To determine the molecular formula of the compound, the empirical formula must be determined first. To determine the empirical formula, the percentage of each constituent is divided by its molar mass. This is shown below

Carbon = 60/12 = 5

Oxygen = 32/16 = 2

Hydrogen = 8/1 = 8

The next step is to divide each ratio by the smallest value. The smallest value is 2. It becomes

Carbon = 5/2 = 2.5

It is approximated to 3

Oxygen = 2/2 = 1

Hydrogen = 8/2 = 4

Therefore, the empirical formula is

C3H4O

From the given relative molecular mass of the compound, the molecular formula can be determined

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.