I need help on my chemistry hw!?

Let % = grams. Find the moles of each and get the simplest ratio by dividing the smaller into the other two.

Moles of carbon = 58.8 / 12 = 4.9

Moles of hydrogen = 9.8 / 1 = 9.8

Moles of oxugen = 31.4 / 16 m= 1.96

Ratio 4.9 / 1.96 = 2.5 9.8 / 1.96 = 5.0 1.96 / 1.96 = 1

Simplest formula = C5H10 )2 Molecular mas is 102. So the simplest fformula inm thjis case is the same.

First of all, the fact that it smells like apples is completely irrelevant. Just getting that out of the way.

Okay. The first thing you want to do is find the empirical formula (the molecular formula in lowest terms):

Start by taking the percents, and taking them to be from a 100 g sample. This means that there is 58.8 g C, 9.8 g H, and 31.4 g O.

Divide each of these by their molar mass

C: 58.8/12.0107 = 4.90

H: 9.8/1.00794 = 9.7

O: 31.4/15.9994 = 1.963

Divide these numbers by the smallest of the lot, in this case, 1.963

C: 4.90/1.963 = 2.50

H: 9.7/1.963 = 4.94 (Just to show something, I didn't round to two sig figs)

O: 1.963/1.963 = 1

Round if the numbers are close to a whole number

C: 2.50

H: 5.0

O: 1

Now multiply everything by the same number such that each of the numbers becomes an integer.

C: 2.50*2 = 5

H: 5.0*2 = 10

O: 1*2 = 2

This is your empirical formula: C5H10O2

Now to get the molecular formula, find the molar mass of your empirical formula.

5(12.0107) + 10(1.00794) + 2(15.9994) = 102.1317 g/mol

In this case, since the molar mass of the empirical formula is the same as the molar mass of the molecular formula, you're done. However, in other scenarios where they are not the same, what you want to do is:

Divide the molar mass of the compound by the molar mass of the compound's empirical formula. Take this number and multiply the subscripts in your empirical formula with it. This will give you your molecular formula.

I'm just going to give an example with a made up compound. Say the empirical formula was...ClO2Si3. The molar mass of this formula would be 151.7083. Now say the actual molar mass of the compound was 455.1249.

455.1249/151.7083 = 3

Multiply each subscript by three: Cl3O6Si9, and you have your molecular formula

C = 58.8g/12.01 = 4.89

H= 9.8/1.01 = 9.70

O = 31.4/16 = 1.96

Take the lowest and divide it by everything

C = 2.49

H = 4.94

O = 1

Times the results by two becasue it is the lowest that makes the numbers whole numbers

C5 H10 O1

Molecular Formula

We are given the Molar mass of methyl butanoate

x = 102/86.15

X= 1.18

C6 H12 O2

CH3-O-CO-C3H7, should be C5H10O2, or

5x12 + 32 + 10 = 102 amu.

However, using the analytical date...

which you should also know how to do...

58.8% C, 9.8% H, and 31.4% O

-------------------------------------------------- gives

12 1 16

C4.9 H9.8 O1.96, or C5 H10 O2

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Its Emprical and molecular formula are same: --> C5H10O2