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Chapter 3: Problem 24

Determine the mass percent of each of the elements in the fungicide copper(II) oleate, $\mathrm{Cu}\left(\mathrm{C}_{18} \mathrm{H}_{33} \mathrm{O}_{2}\right)_{2}$

Short Answer

Expert verified
The mass percent of each element in Copper(II) oleate can be determined by the method of calculating mass percent using atomic masses and mole concept. The mass percent of an element = (mass of the element in one mole of the compound / molar mass of the compound) x 100. It's necessary to compute the molar mass of Copper(II) oleate as the first step, and then use it to calculate the mass percent of each element.

Step by step solution

01

Determine the Molecular Mass of Copper(II) Oleate

Molecular weight of Copper(II) oleate, Cu(C18H33O2)2 can be calculated by adding the atomic masses of its constituent atoms. It is important to use the correct atomic weights in atomic mass units (amu). The atomic weights of copper, carbon, hydrogen, and oxygen are 63.55 amu, 12.01 amu, 1.01 amu, and 16.00 amu respectively. Then multiply each of these by the number of each atom in the molecule and sum up the results. So, the molecular weight of Copper(II) oleate = 63.55 + 2*[(18*12.01) + (33*1.01) + (2*16.00)] amu.
02

Calculate the Mass Percent

The mass percent of an element is calculated by dividing the total mass of each element in one molecule by the molar mass of copper(II) oleate. Then, multiply the result by 100 to get a percentage. The formulas are as follows: \%Cu = [mass of Cu / molar mass of copper(II) oleate] x100. \%C = [mass of C / molar mass of copper(II) oleate] x100. \%H = [mass of H / molar mass of copper(II) oleate] x100. \%O = [mass of O / molar mass of copper(II) oleate] x100.
03

Execute the Calculations

Now substitute the earlier determined values into the respective formulas to find out the mass percentages of copper, carbon, hydrogen, and oxygen in copper(II) oleate.

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Most popular questions from this chapter

Malachite is a common copper-containing mineral with the formula \(\mathrm{CuCO}_{3} \cdot \mathrm{Cu}(\mathrm{OH})_{2} .\) (a) What is the mass percent copper in malachite? (b) When malachite is strongly heated, carbon dioxide and water are driven off, yielding copper(II) oxide as the sole product. What mass of copper(II) oxide is produced per kg of malachite?

The mineral spodumene has the empirical formula \(\mathrm{LiAlSi}_{2} \mathrm{O}_{6} .\) Given that the percentage of lithium- 6 atoms in naturally occuring lithium is \(7.40 \%,\) how many lithium- 6 atoms are present in a 518 g sample of spodumene?

Without doing detailed calculations, explain which of these compounds produces the greatest mass of \(\mathrm{H}_{2} \mathrm{O}\) when \(1.00 \mathrm{g}\) of the compound is burned in an excess of oxygen: \(\mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{C}_{10} \mathrm{H}_{8}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\)

Some substances that are only very slightly soluble in water will spread over the surface of water to produce a film that is called a monolayer because it is only one molecule thick. A practical use of this phenomenon is to cover ponds to reduce the loss of water by evaporation. Stearic acid forms a monolayer on water. The molecules are arranged upright and in contact with one another, rather like pencils tightly packed and standing upright in a coffee mug. The model below represents an individual stearic acid molecule in the monolayer. (a) How many square meters of water surface would be covered by a monolayer made from \(10.0 \mathrm{g}\) of stearic acid? [Hint: What is the formula of stearic acid?] (b) If stearic acid has a density of \(0.85 \mathrm{g} / \mathrm{cm}^{3}\), estimate the length (in nanometers) of a stearic acid molecule. [Hint: What is the thickness of the monolayer described in part a?] (c) A very dilute solution of oleic acid in liquid pentane is prepared in the following way: $$\begin{aligned} &1.00 \mathrm{mL} \text { oleic acid }+9.00 \mathrm{mL} \text { pentane } \rightarrow \text { solution }(1)\\\ &1.00 \mathrm{mL} \text { solution }(1)+9.00 \mathrm{mL} \text { pentane } \rightarrow \text { solution }(2)\\\ &1.00 \mathrm{mL} \text { solution }(2)+9.00 \mathrm{mL} \text { pentane } \rightarrow \text { solution }(3)\\\ &1.00 \mathrm{mL} \text { solution }(3)+9.00 \mathrm{mL} \text { pentane } \rightarrow \text { solution }(4) \end{aligned}$$ A 0.10 mL sample of solution (4) is spread in a monolayer on water. The area covered by the monolayer is \(85 \mathrm{cm}^{2} .\) Assume that oleic acid molecules are arranged in the same way as described for stearic acid, and that the cross-sectional area of the molecule is \(4.6 \times 10^{-15} \mathrm{cm}^{2}\). The density of oleic acid is \(0.895 \mathrm{g} / \mathrm{mL} .\) Use these data to obtain an approximate value of Avogadro's number.

Adenine, a component of nucleic acids, has the mass percent composition: \(44.45 \%\) C \(, 3.73 \%\) H, \(51.82 \%\) N. Its molecular mass is 135.14 u. What is its molecular formula?
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