Chemistry : asked on johnsnow69

17.06.2021

Given the empirical formula C2H3O, what is the molecular formula that has a mass of 214.8g?

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09.07.2023, solved by verified expert

Mathematics, DAV Post Graduate College

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Given the empirical formula, the molecular formula that has a mass of 214.8g is C₁₀H₁₅O₅

Empirical & ,molecular formulae

From the question, we are to determine the molecular formula

From

Molecular formula = (Empirical formula)n

Where

From the given information,

Empirical formula is C₂H₃O

Therefore, Empirical formula mass = (12×2) + (1×3) + (16)

Empirical formula mass = 24 + 3 + 16

Empirical formula mass = 40 g

Then,

n = 5.37

n ≅ 5

Therefore,

Molecular formula = (C₂H₃O)₅

Molecular formula = C₁₀H₁₅O₅

Hence, given the empirical formula, the molecular formula that has a mass of 214.8g is C₁₀H₁₅O₅

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Chemistry

Given the empirical formula C2H3O, what is the molecular formula that has a mass of 214.8g?

Step-by-step answer

P Answered by Master

Given the empirical formula, the molecular formula that has a mass of 214.8g is C₁₀H₁₅O₅

Empirical & ,molecular formulae

From the question, we are to determine the molecular formula

From

Molecular formula = (Empirical formula)n

Where

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

From the given information,

Empirical formula is C₂H₃O

Therefore, Empirical formula mass = (12×2) + (1×3) + (16)

Empirical formula mass = 24 + 3 + 16

Empirical formula mass = 40 g

Then,

$n = \frac{214.8}{40}$

n = 5.37

n ≅ 5

Therefore,

Molecular formula = (C₂H₃O)₅

Molecular formula = C₁₀H₁₅O₅

Hence, given the empirical formula, the molecular formula that has a mass of 214.8g is C₁₀H₁₅O₅

Learn more on Empirical and molecular formulae here:

Chemistry

Please help :) A compound has the empirical formula C2H3O and a molecular mass of 172 mol. What is its molecular formula? a. C11H10 05 b. C6H9O3 c. C8H12O4 d. C4H6O2

Step-by-step answer

P Answered by Specialist

Empirical formula mass :-

$\\ \tt\Rrightarrow C_2H_3O$

$\\ \tt\Rrightarrow 24+16+3=43g/mol$

n:-

Molar mass/Empirical formula mass

$\\ \tt\Rrightarrow \dfrac{172}{43}$

$\\ \tt\Rrightarrow 4$

Molecular formula

4(C_2H_3O)=C_8H_12O_4

Chemistry

Please help :) A compound has the empirical formula C2H3O and a molecular mass of 172 mol. What is its molecular formula? a. C11H10 05 b. C6H9O3 c. C8H12O4 d. C4H6O2

Step-by-step answer

P Answered by Specialist

Empirical formula mass :-

$\\ \tt\Rrightarrow C_2H_3O$

$\\ \tt\Rrightarrow 24+16+3=43g/mol$

n:-

Molar mass/Empirical formula mass

$\\ \tt\Rrightarrow \dfrac{172}{43}$

$\\ \tt\Rrightarrow 4$

Molecular formula

4(C_2H_3O)=C_8H_12O_4

Chemistry

17. which of the following is not an empirical formula? * a. sb2s3 b. c2h3o c. beso4 d. c2h6 18. which of the following is not true comparing empirical and molecular formulas? * a. the molecular formula can be a simple whole number multiple of the empirical formula. b. the molecular formula of a compound can identical to its empirical formula. c. the empirical formula of a compound can be twice the molecular formula. d. several compounds can start with the same empirical formula, but have different molecular formulas.

Step-by-step answer

P Answered by PhD

6

17) d. C_2H_6

18. c. The empirical formula of a compound can be twice the molecular formula.

Explanation:

Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.

To calculate the molecular formula, we need to find the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

The empirical mass can be calculated from empirical formula and molar mass must be known.

17. Thus the empirical formula of C_2H_6 should be CH_3

18. The molecular formula will either be same as empirical formula or is a whole number multiple of empirical formula. Thus the empirical formula of a compound can never be twice the molecular formula.

Chemistry

17. which of the following is not an empirical formula? * a. sb2s3 b. c2h3o c. beso4 d. c2h6 18. which of the following is not true comparing empirical and molecular formulas? * a. the molecular formula can be a simple whole number multiple of the empirical formula. b. the molecular formula of a compound can identical to its empirical formula. c. the empirical formula of a compound can be twice the molecular formula. d. several compounds can start with the same empirical formula, but have different molecular formulas.

Step-by-step answer

P Answered by PhD

6

17) d. C_2H_6

18. c. The empirical formula of a compound can be twice the molecular formula.

Explanation:

Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.

To calculate the molecular formula, we need to find the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

The empirical mass can be calculated from empirical formula and molar mass must be known.

17. Thus the empirical formula of C_2H_6 should be CH_3

18. The molecular formula will either be same as empirical formula or is a whole number multiple of empirical formula. Thus the empirical formula of a compound can never be twice the molecular formula.

Chemistry

Severus Snape explains that if you have the molar mass of a compound and the empirical formula of a compound you can determine the molecular formula of a compound. Suppose you have a compound which has an empirical formula of C2H3O and molar mass of 86 g/mol. What is the compounds molecular formula

Step-by-step answer

P Answered by Master

The molecular formula of the compound : C_4H_6O_2

Explanation:

The empirical formula of the compound = C_2H_3O

The molecular formula of the compound = $C_{2n}H_{3n}O_n$

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Mass of molecular formula = 86 g/mol

Mass of empirical formula = 43 g/mol

Putting values in above equation, we get:

$n=\frac{86g/mol}{43g/mol}=2$

The molecular formula of the compound :

$C_{2\times 2}H_{3\times 2}O_2=C_4H_6O_2$

Chemistry

Severus Snape explains that if you have the molar mass of a compound and the empirical formula of a compound you can determine the molecular formula of a compound. Suppose you have a compound which has an empirical formula of C2H3O and molar mass of 86 g/mol. What is the compounds molecular formula

Step-by-step answer

P Answered by Specialist

The molecular formula of the compound : C_4H_6O_2

Explanation:

The empirical formula of the compound = C_2H_3O

The molecular formula of the compound = $C_{2n}H_{3n}O_n$

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Mass of molecular formula = 86 g/mol

Mass of empirical formula = 43 g/mol

Putting values in above equation, we get:

$n=\frac{86g/mol}{43g/mol}=2$

The molecular formula of the compound :

$C_{2\times 2}H_{3\times 2}O_2=C_4H_6O_2$

Chemistry

A molecule has the empirical formula C4H6O. If its molecular weight is determined to be about 212 g/mol, what is the most likely molecular formula? a. C12H18O3 b. C8H12O3 c. C11H16O4 d. C4H6O e. C2H3O

Step-by-step answer

P Answered by PhD

1

The molecular formula is C12H18O3

Explanation:

Step 1: Data given

The empirical formula is C4H6O

Molecular weight is 212 g/mol

atomic mass of C = 12 g/mol

atomic mass of H = 1 g/mol

atomic mass of O = 16 g/mol

Step 2: Calculate the molar mass of the empirical formula

Molar mass = 4* 12 + 6*1 +16

Molar mass = 70 g/mol

Step 3: Calculate the molecular formula

We have to multiply the empirical formula by n

n = the molecular weight of the empirical formula / the molecular weight of the molecular formula

n = 70 /212 ≈ 3

We have to multiply the empirical formula by 3

3*(C4H6O- = C12H18O3

The molecular formula is C12H18O3

Chemistry

A molecule has the empirical formula C4H6O. If its molecular weight is determined to be about 212 g/mol, what is the most likely molecular formula? a. C12H18O3 b. C8H12O3 c. C11H16O4 d. C4H6O e. C2H3O

Step-by-step answer

P Answered by PhD

1

The molecular formula is C12H18O3

Explanation:

Step 1: Data given

The empirical formula is C4H6O

Molecular weight is 212 g/mol

atomic mass of C = 12 g/mol

atomic mass of H = 1 g/mol

atomic mass of O = 16 g/mol

Step 2: Calculate the molar mass of the empirical formula

Molar mass = 4* 12 + 6*1 +16

Molar mass = 70 g/mol

Step 3: Calculate the molecular formula

We have to multiply the empirical formula by n

n = the molecular weight of the empirical formula / the molecular weight of the molecular formula

n = 70 /212 ≈ 3

We have to multiply the empirical formula by 3

3*(C4H6O- = C12H18O3

The molecular formula is C12H18O3

Chemistry

What elements combined with Strontium, St, in a 1:1 ratio?

Step-by-step answer

P Answered by PhD

Answer: chalcogens.
Explanation: Strontium is an alkaline earth metal, it always exhibits a degree of oxidation in its compounds +2.
Chalcogens are a group of 6 chemical elements (oxygen O, sulfur S, selenium se, tellurium te, polonium Po) that have an oxidation state of -2 => Chalcogens will combine with strontium in a ratio of 1:1.

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