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Chapter 3: Problem 46

The organic solvent thiophene is a carbon-hydrogensulfur compound that yields \(\mathrm{CO}_{2}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{SO}_{2}\) when burned in an excess of oxygen. When subjected to combustion analysis, a \(1.3020 \mathrm{g}\) sample of thiophene produces \(2.7224 \mathrm{g} \mathrm{CO}_{2}, 0.5575 \mathrm{g} \mathrm{H}_{2} \mathrm{O},\) and \(0.9915 \mathrm{g} \mathrm{SO}_{2} .\) What is the empirical formula of thiophene?

Short Answer

Expert verified
The empirical formula of thiophene is \(\mathrm{C}_4\mathrm{H}_4\mathrm{S}\).

Step by step solution

01

Determine the Masses of C, H and S

From the combustion, 2.7224g of \(\mathrm{CO}_2\) gives the mass of C as: \((12.01 / 44.01) \times 2.7224 \mathrm{g}\) \(\mathrm{CO}_2\). H from 0.5575g \(\mathrm{H}_2\mathrm{O}\) is: \((2.016 / 18.015) \times 0.5575 \mathrm{g}\) \(\mathrm{H}_2\mathrm{O}\). And S from 0.9915g \(\mathrm{SO}_2\) is: \((32.065 / 64.066) \times 0.9915 \mathrm{g}\) \(\mathrm{SO}_2\).
02

Calculate the Number of Moles

The number of moles is given by the mass divided by the molar mass. Calculate the number of moles for C, H, and S using their respective molar masses of 12.01 g/mol, 1.008 g/mol, and 32.065 g/mol.
03

Determine the Empirical Formula

To determine the empirical formula, divide each of the number of moles calculated by the smallest number obtained. Then, round to the nearest whole number to get the ratio and therefore the formula.

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Most popular questions from this chapter

A piece of gold (Au) foil measuring \(0.25 \mathrm{mm} \times\) \(15 \mathrm{mm} \times 15 \mathrm{mm}\) is treated with fluorine gas. The treatment converts all the gold in the foil to \(1.400 \mathrm{g}\) of a gold fluoride. What is the formula and name of the fluoride? The density of gold is \(19.3 \mathrm{g} / \mathrm{cm}^{3}\)

Determine the mass percent of each of the elements in the antimalarial drug quinine, \(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{2}\)

\(\mathrm{MgCl}_{2}\) often occurs in table salt \((\mathrm{NaCl})\) and is responsible for caking of the salt. A 0.5200 g sample of table salt is found to contain \(61.10 \%\) Cl, by mass. What is the \(\% \mathrm{MgCl}_{2}\) in the sample? Why is the precision of this calculation so poor?

Para-cresol ( \(p\) -cresol) is used as a disinfectant and in the manufacture of herbicides. A 0.4039 g sample of this carbon-hydrogen-oxygen compound yields \(1.1518 \mathrm{g} \mathrm{CO}_{2}\) and \(0.2694 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) in combustion analysis. Its molecular mass is 108.1 u. For \(p\) -cresol, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.

Dimethylhydrazine is a carbon-hydrogen-nitrogen compound used in rocket fuels. When burned in an excess of oxygen, a \(0.312 \mathrm{g}\) sample yields \(0.458 \mathrm{g} \mathrm{CO}_{2}\) and \(0.374 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\). The nitrogen content of a \(0.486 \mathrm{g}\) sample is converted to \(0.226 \mathrm{g} \mathrm{N}_{2} .\) What is the empirical formula of dimethylhydrazine?
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