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Chapter 3: Problem 20

Determine the mass percent \(O\) in the mineral malachite, \(\mathrm{Cu}_{2}(\mathrm{OH})_{2} \mathrm{CO}_{3}\)

Short Answer

Expert verified
The mass percent of Oxygen in the mineral malachite is approximately 28.94%.

Step by step solution

01

Determine the Molar Mass of the Mineral

To calculate the molar mass of the mineral Malachite (\(\mathrm{Cu}_{2}(\mathrm{OH})_{2} \mathrm{CO}_{3}\)), the molar masses of its constituents must be added together. The molar mass of Copper (Cu) is approximately 63.55 g/mol, that of Oxygen (O) is 16.00 g/mol and Hydrogen (H) is 1.01 g/mol. Carbon (C) has a molar mass of 12.01 g/mol. Thus, the molar mass of Malachite is given by: \2(63.55 g/mol) + 2(16.00 g/mol + 1.01 g/mol) + 3(16.00 g/mol) + 12.01 g/mol = 221.12 g/mol.
02

Calculate Total Molar Mass of Oxygen in the Mineral

There are 4 Oxygen atoms in one formula unit of Malachite: two in the hydroxide (\(\mathrm{OH}\)) ions and two in the carbonate (\(\mathrm{CO}_{3}\)) ion. Therefore, total molar mass of Oxygen in the mineral is: \4 * 16.00 g/mol = 64.00 g/mol.
03

Calculate the Mass Percent of Oxygen

The mass percent of Oxygen can now be calculated from the molar mass of Oxygen and the total molar mass of the compound: \\(Mass\,Percent\,Oxygen = \frac{Total\,Oxygen\,Molar\,Mass}{Molar\,Mass\,of\,Malachite} * 100% = \frac{64.00\,g/mol}{221.12\,g/mol} * 100% ≈ 28.94% \)

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Most popular questions from this chapter

\(\mathrm{MgCl}_{2}\) 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?

Diethylene glycol, used to deice aircraft, is a carbonhydrogen-oxygen compound with \(45.27 \%\) C and \(9.50 \%\) H by mass. What is its empirical formula?

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?

The atomic mass of \(\mathrm{Bi}\) is to be determined by converting the compound \(\mathrm{Bi}\left(\mathrm{C}_{6} \mathrm{H}_{5}\right)_{3}\) to \(\mathrm{Bi}_{2} \mathrm{O}_{3} .\) If \(5.610 \mathrm{g}\) of \(\mathrm{Bi}\left(\mathrm{C}_{6} \mathrm{H}_{5}\right)_{3}\) yields \(2.969 \mathrm{g} \mathrm{Bi}_{2} \mathrm{O}_{3},\) what is the atomic mass of Bi?

Without doing detailed calculations, arrange the following in order of increasing \(\% \mathrm{Cr},\) by mass, and explain your reasoning: \(\mathrm{CrO}, \mathrm{Cr}_{2} \mathrm{O}_{3}, \mathrm{CrO}_{2}, \mathrm{CrO}_{3}\)
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