Chemistry, 02.03.2020 06:38 gacyber

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

Answers: 1

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Answer from: dominickstrickland

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

Answer from: jnthnsngh

The molecular formula is most likely to be first option, $\rm C_{12} H_{18} O_{3}$ .

Explanation:

Both the molecular formula and the empirical formula of a molecule give the types of atoms in that molecule. However, the molecular formula of a molecule gives the exact number of atoms each molecule. On the other hand, the empirical formula gives only a simplified ratio.

For example, if the empirical formula of the molecule is $\rm C_4H_6O$ , then the molecular formula would be $(\rm C_4H_6O)_k$ , or equivalently $\mathrm{C}_{4\, k}\mathrm{H}_{6\, k} \mathrm{O}_{k}$ , where is a positive whole number ( $1,\, 2,\, \dots$ , etc.) The goal here is to find the value of

Look up the relative atomic mass data on a modern periodic table:

C: 12.011.H: 1.008.O: 15.999.

The formula mass of $\rm C_4 H_6 O$ would be

$\begin{aligned}&M(\rm C_4 H_6 O) \cr &\approx 4 \times 12.011 + 6 \times 1.008 + 15.999 \cr &= 70.091\;\rm g \cdot mol^{-1}\end{aligned}$ .

The formula mass of $\mathrm{C}_{4\, k}\mathrm{H}_{6\, k} \mathrm{O}_{k}$ would be

$\begin{aligned}&M(\mathrm{C}_{4\, k}\mathrm{H}_{6\, k} \mathrm{O}_{k}) \cr &\approx (4\, k) \times 12.011 + (6\, k) \times 1.008 + k \times 15.999 \cr &= ( 4 \times 12.011 + 6 \times 1.008 + 15.999)\, k \\ &= (70.091\, k)\;\rm g \cdot mol^{-1}\end{aligned}$ .

On the other hand, since the molecule should have a molecular mass of $\rm 212\; g \cdot mol^{-1}$ ,

$70.091\, k \approx 212$ .

$k \approx 3$ . (Round to the nearest whole number.)

Hence, the molecular formula would be $\rm C_{(4 \times 3)} H_{(6 \times 3)}O_{3}$ , which simplifies to $\rm C_{12} H_{18} O_{3}$ .

Answer from: Quest

consider the reaction below.

no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

Answer from: Quest

The formula is (nh4)2co3

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A molecule has the empirical formula C4H6O. If its molecular weight is determined to be about 212 g/...