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Chapter 3: Problem 125

A formula unit of the compound \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) has nearly equal masses of (a) \(\mathrm{S}\) and \(\mathrm{O} ;\) (b) \(\mathrm{N}\) and \(\mathrm{O}\) (c) \(\mathrm{H}\) and \(\mathrm{N} ;\) (d) \(\mathrm{Cu}\) and \(\mathrm{O}\)

Short Answer

Expert verified
For none of the pairs a, b, c, d, the masses are nearly equal in the given compound.

Step by step solution

01

List the atomic masses

Look up and list the atomic masses of the involved elements. The numbers are approximate: S (sulfur) = 32 g/mol, O (oxygen) = 16 g/mol, N (nitrogen) = 14 g/mol, H (hydrogen) = 1 g/mol, and Cu (copper) = 63.5 g/mol.
02

Calculate the masses of each element in the formula

Using the chemical formula \([\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\), calculate the total mass of each constituent in one formula unit. For S, it's 32 g/mol. For O, it occurs five times (four in SO4 and one in Cu), so its mass is 5*16 = 80 g/mol. For N, it is in 4 NH3 groups, so its mass is 4*14 = 56 g/mol. H is in the 4 NH3 groups, its mass is 4*3*1 = 12 g/mol (each NH3 has 3 H atoms). Cu has a mass of 63.5 g/mol.
03

Compare the masses

Compare the masses pairwise, as stated in the exercise. For a, S = 32 g/mol, O = 80 g/mol, not equal. For b, N = 56 g/mol, O = 80 g/mol, not equal. For c, H = 12 g/mol, N = 56 g/mol, not equal. For d, Cu = 63.5 g/mol, O = 80 g/mol, not equal.

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Most popular questions from this chapter

Explain which of the following statement(s) is (are) correct for sorbic acid, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{2},\) an inhibitor of mold and yeast. (a) It has a \(\mathrm{C}: \mathrm{H}:\) O mass ratio of 3: 4: 1 (b) It has the same mass percent composition as the aquatic herbicide, acrolein, \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}\) (c) It has the same empirical formula as aspidinol, \(\mathrm{C}_{12} \mathrm{H}_{16} \mathrm{O}_{4},\) a drug used to kill parasitic worms. (d) It has four times as many \(\mathrm{H}\) atoms as \(\mathrm{O}\) atoms, but four times as much O as H by mass.

Determine the empirical formula of (a) the rodenticide (rat killer) warfarin, which consists of \(74.01 \% \mathrm{C}\) \(5.23 \% \mathrm{H},\) and \(20.76 \%\) O, by mass; (b) the antibacterial agent sulfamethizole, which consists of \(39.98 \%\) C. \(3.73 \% \mathrm{H}, 20.73 \% \mathrm{N}, 11.84 \% \mathrm{O},\) and \(23.72 \% \mathrm{S},\) by mass.

Explain which of the following statement(s) is (are) correct concerning glucose (blood sugar), \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (a) The percentages, by mass, of \(\mathrm{C}\) and \(\mathrm{O}\) are the same as in CO. (b) The ratio of \(\mathrm{C}: \mathrm{H}: \mathrm{O}\) atoms is the same as in dihydroxyacetone, \(\left(\mathrm{CH}_{2} \mathrm{OH}\right)_{2} \mathrm{CO}\) (c) The proportions, by mass, of \(C\) and \(O\) are equal. (d) The highest percentage, by mass, is that of H.

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

All-purpose fertilizers contain the essential elements nitrogen, phosphorus, and potassium. A typical fertilizer carries numbers on its label, such as "5-10-5". These numbers represent the \% \(\mathrm{N}, \% \mathrm{P}_{2} \mathrm{O}_{5},\) and \(\% \mathrm{K}_{2} \mathrm{O},\) respectively. The \(\mathrm{N}\) is contained in the form of a nitrogen compound, such as \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}, \mathrm{NH}_{4} \mathrm{NO}_{3}\) or \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\) (urea). The \(\mathrm{P}\) is generally present as a phosphate, and the \(K\) as \(K C\). The expressions \(\% \mathrm{P}_{2} \mathrm{O}_{5}\) and \(\% \mathrm{K}_{2} \mathrm{O}\) were devised in the nineteenth century, before the nature of chemical compounds was fully understood. To convert from \% \(\mathrm{P}_{2} \mathrm{O}_{5}\) to \% \(\mathrm{P}\) and from \% \(\mathrm{K}_{2} \mathrm{O}\) to \% \(\mathrm{K}\), the factors \(2 \mathrm{mol} \mathrm{P} / \mathrm{mol}\) \(\mathrm{P}_{2} \mathrm{O}_{5}\) and \(2 \mathrm{mol} \mathrm{K} / \mathrm{mol} \mathrm{K}_{2} \mathrm{O}\) must be used, together with molar masses. (a) Assuming three-significant-figure precision, what is the percent composition of the "5-10-5" fertilizer in \% \(\mathrm{N}, \% \mathrm{P},\) and \(\% \mathrm{K} ?\) (b) What is the \(\% \mathrm{P}_{2} \mathrm{O}_{5}\) in the following compounds (both common fertilizers)? (i) \(\mathrm{Ca}\left(\mathrm{H}_{2} \mathrm{PO}_{4}\right)_{2}\) (ii) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) (c) In a similar manner to the "5-10-5" fertilizer described in this exercise, how would you describe a fertilizer in which the mass ratio of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) to KCl is 5.00:1.00? (d) Can a "5-10-5" fertilizer be prepared in which \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) and \(\mathrm{KCl}\) are the sole fertilizer components, with or without inert nonfertilizer additives? If so, what should be the proportions of the constituents of the fertilizer mixture? If this "5-10-5" fertilizer cannot be prepared, why not?
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