Chemistry, 07.03.2020 03:46 dakotaadkins20

3.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 136. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured product mass water .59 g Use this information to find the molecular formula of X.

Answers: 2

Show answers

Answers

Answer from: gracethegreat1

The question is incomplete, here is the complete question:

3.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 136. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured:

Product Mass

Carbon dioxide 7.77 g

Water 1.59 g

Use this information to find the molecular formula of X.

The molecular formula for the given organic compound is C_8H_8O_2

Explanation:

We are given:

Mass of CO_2=7.77g

Mass of H_2O=1.59g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 7.77 g of carbon dioxide, $\frac{12}{44}\times 7.77=2.12g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 1.59 g of water, $\frac{2}{18}\times 1.59=0.176g$ of hydrogen will be contained.

Mass of oxygen in the compound = (3.00) - (2.12 + 0.176) = 0.704 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{2.12g}{12g/mole}=0.176moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.176g}{1g/mole}=0.176moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.704g}{16g/mole}=0.044moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.044 moles.

For Carbon = $\frac{0.176}{0.044}=4$

For Hydrogen = $\frac{0.176}{0.044}=4$

For Oxygen = $\frac{0.044}{0.044}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 4 : 4 : 1

The empirical formula for the given compound is C_4H_4O

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 68 g/mol

Mass of empirical formula = 136 g/mol

Putting values in above equation, we get:

$n=\frac{136g/mol}{68g/mol}=2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(4\times 2)}H_{(4\times 2)}O_{(1\times 2)}=C_8H_8O_2$

Hence, the molecular formula for the given organic compound is C_8H_8O_2

Answer from: Quest

"the periodic table is arranged in order of atomic number."

Answer from: Quest

Yes you are correct use the scientific method

Another question on Chemistry

Chemistry, 22.06.2019 07:10

An experimental procedure requires a 10 ml of acid to be dissolved

Answers: 2

Answer

Chemistry, 22.06.2019 08:30

Agroup of students is studying convection current. they fill two identical balloons with the same amount of helium. one balloon is placed in a freezer and the other is in an area with warm air. after 10 minutes, the balloon are released from a height of 1 meter. which of the following to the students most likely observe? a) the warm balloon expands and rises. the cold balloon shrinks and sinks b) the balloon both rise. the cold balloon is larger than the warm balloon c) the cold balloon expands and rises. the warm balloon shrinks and sinks d) the balloon rise at the same rate. both balloons are the same size

Answers: 1

Answer

Chemistry, 22.06.2019 08:30

Which of the following would have less momentum than a 52 kg cheetah running at 10 m/s?

Answers: 2

Answer

Chemistry, 23.06.2019 00:00

What is the approximate mass of 25 cm3 of silver, if the density is 10.5 g/cm3? a. 0.42 g b. 2.4 g c. 42 g d. 260 g

Answers: 1

Answer

You know the right answer?

3.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have...