Chemistry , 21.06.2019 18:00 mykalwashington

The compound methyl butanoate smells like apples. its percent composition is 58.8% c, 9.9% h, and 31.4% o. what’s the empirical formula ?

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Answer from: stephanielynch

To find the empirical formula you would first need to find the moles of each element:

58.8g/ 12.0g = 4.9 mol C

9.9g/ 1.0g = 9.9 mol H

31.4g/ 16.0g = 1.96 O

Then you divide by the smallest number of moles of each:

4.9/1.96 = 2.5

9.9/1.96 = 6

1.96/1.96 = 1

Since there is 2.5, you find the least number that makes each moles a whole number which is 2.

So the empirical formula is C5H12O2.

Answer from: sidney2602

Answer : The empirical and molecular formula of the compound is,

Solution :

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C = 58.8 g

Mass of H = 9.8 g

Mass of O = 31.4 g

Molar mass of C = 12 g/mole

Molar mass of H = 1 g/mole

Molar mass of O = 16 g/mole

Step 1 : convert given masses into moles.

Moles of C =

Moles of H =

Moles of O =

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =

For H =

For O =

The ratio of C : H : O = 2.5 : 5 : 1

To make the ratio in a whole number we are multiplying ratio by 2, we get:

The ratio of C : H : O = 5 : 10 : 2

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula =

The empirical formula weight = 5(12) + 10(1) + 2(16) = 102 gram/eq

Now we have to calculate the molecular formula of the compound.

Formula used :

Molecular formula =

Therefore, the molecular formula of the compound is,

Answer from: izeahzapata1

Let our basis for the calculation be 1 mol of the substance.
(1 mol)(102 g/mol) = 102 g
Determine the amount of C, H, and O in mole.
C = (102 g)(0.588)(1 mol/12 g) = 4.998 mols C
H = (102 g)(0.098)(1 mol/1 g) = 9.996 mols H
O = (102 g)(0.314)(1 mol/16 g) = 2 mols O

The empirical formula of the substance is C5H10O2. The molar mass of the empirical formula is 102. This means that this is also its molecular formula.

Answer from: pbargy9551

CH3OCOC3H7 or

O2C5H10

Explanation:

Assuiming a 100 g sample,

58.8g C / (1 mole/12g) = 4.9 moles C

9.8gH / (1 mole/1g) = 9.8 moles H

31.4 gO / (1mole/16g) = 1.96 moles O

4.9 moles C/1.96 = 2.5moles C x 2 = 5moles C

9.8 moles H/1.96 = 5 moles H x 2 = 10 moles H

1.96 moles O/1.96 = 1 mole O x 2= moles O

C5H10O2

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