Organic compounds called carbobydrates may be formed in...

Organic compounds called carbobydrates may be formed in reactions between iron(II) sulfide and carbonic acid: $$2 \mathrm{FeS}+\mathrm{H}_{2} \mathrm{CO}_{3} \rightarrow 2 \mathrm{FeO}+\frac{1}{n}\left(\mathrm{CH}_{2} \mathrm{O}\right)_{n}+2 \mathrm{S}$$ a. What is the empirical formula of these carbohydrates? b. How much carbohydrate is produced from a reaction mixture that initially contains $211 \mathrm{g}$ FeS and excess $\mathrm{H}_{2} \mathrm{CO}_{3}$ if the reaction results in a $78.5 \%$ yield? c. If the carbohydrate product has a molecular mass of 300 amu, what is its molecular formula?

Organic compounds called carbobydrates may be formed in reactions between iron(II) sulfide and carbonic acid:
$$2 \mathrm{FeS}+\mathrm{H}_{2} \mathrm{CO}_{3} \rightarrow 2 \mathrm{FeO}+\frac{1}{n}\left(\mathrm{CH}_{2} \mathrm{O}\right)_{n}+2 \mathrm{S}$$
a. What is the empirical formula of these carbohydrates?
b. How much carbohydrate is produced from a reaction mixture that initially contains $211 \mathrm{g}$ FeS and excess $\mathrm{H}_{2} \mathrm{CO}_{3}$ if the reaction results in a $78.5 \%$ yield?
c. If the carbohydrate product has a molecular mass of 300 amu, what is its molecular formula?

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Key Concepts

Percent Yield

Percent yield is a practical measure of a chemical reaction’s efficiency. It compares the experimentally obtained amount of product to the theoretical amount predicted by stoichiometry, expressed as a percentage. This concept is essential in assessing reaction performance and determining the practicality of chemical syntheses.

Stoichiometry

Stoichiometry is the quantitative analysis of reactants and products in a chemical reaction. It uses the coefficients of the balanced chemical equation to relate the amounts of substances that participate in the reaction, and it is fundamental for calculating yields and conversions in both laboratory and industrial processes.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the elements present in a compound. In carbohydrates, this typically results in the ratio CH2O, indicating that each unit contains one carbon, two hydrogens, and one oxygen, regardless of the actual size of the molecule.

Molecular Formula Determination

Determining the molecular formula involves finding the actual numbers of each atom in a molecule. This is achieved by using the empirical formula as a reference and incorporating the molar mass of the molecule to see how many times the empirical unit is repeated in the molecular structure.

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