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Chapter 3: Problem 162

Consider samples of phosphine \(\left(\mathrm{PH}_{3}\right),\) water \(\left(\mathrm{H}_{2} \mathrm{O}\right),\) hydrogen sulfide \(\left(\mathrm{H}_{2} \mathrm{S}\right),\) and hydrogen fluoride (HF), each with a mass of 119 \(\mathrm{g} .\) Rank the compounds from the least to the greatest number of hydrogen atoms contained in the samples.

Short Answer

Expert verified
The samples rank from the least to the greatest number of hydrogen atoms as follows: Hydrogen fluoride (HF) with 5.95 moles of H, hydrogen sulfide (H2S) with 6.98 moles of H, phosphine (PH3) with 10.5 moles of H, and water (H2O) with 13.22 moles of H: HF < H2S < PH3 < H2O.

Step by step solution

01

Calculate the molar mass of each compound

First, we need to find the molar mass of the compounds given: For phosphine (PH3): Molar mass = (1 x P) + (3 x H) = \(1 \times 30.97 + 3 \times 1.01 = 34\ \mathrm{g/mol}\) For water (H2O): Molar mass = (2 x H) + (1 x O) = \(2 \times 1.01 + 1 \times 16.00 = 18\ \mathrm{g/mol}\) For hydrogen sulfide (H2S): Molar mass = (2 x H) + (1 x S) = \(2 \times 1.01 + 1 \times 32.07 = 34.09\ \mathrm{g/mol}\) For hydrogen fluoride (HF): Molar mass = (1 x H) + (1 x F) = \(1 \times 1.01 + 1 \times 19.00 = 20.01\ \mathrm{g/mol}\)
02

Determine the number of moles of each compound in the samples

Now we need to find the number of moles of each compound in the 119 gram samples. For phosphine (PH3): Moles = \(\frac{Mass}{Molar\ mass} = \frac{119}{34} = 3.5\ \mathrm{moles}\) For water (H2O): Moles = \(\frac{119}{18} = 6.61\ \mathrm{moles}\) For hydrogen sulfide (H2S): Moles = \(\frac{119}{34.09} = 3.49\ \mathrm{moles}\) For hydrogen fluoride (HF): Moles = \(\frac{119}{20.01} = 5.95\ \mathrm{moles}\)
03

Calculate the number of moles of hydrogen atoms for each compound

Now, we need to find the number of moles of hydrogen atoms in each compound. For phosphine (PH3): Moles of hydrogen = \(3.5\ \mathrm{moles\ (PH3)} \times 3\ \mathrm{H\ atoms} = 10.5\ \mathrm{moles\ of\ H}\) For water (H2O): Moles of hydrogen = \(6.61\ \mathrm{moles\ (H2O)} \times 2\ \mathrm{H\ atoms} = 13.22\ \mathrm{moles\ of\ H}\) For hydrogen sulfide (H2S): Moles of hydrogen = \(3.49\ \mathrm{moles\ (H2S)} \times 2\ \mathrm{H\ atoms} = 6.98\ \mathrm{moles\ of\ H}\) For hydrogen fluoride (HF): Moles of hydrogen = \(5.95\ \mathrm{moles\ (HF)} \times 1\ \mathrm{H\ atom} = 5.95\ \mathrm{moles\ of\ H}\)
04

Compare and rank the compounds based on the number of moles of hydrogen atoms

Now that we have the number of moles of hydrogen atoms for each compound, we can compare and rank them. From least to greatest number of moles of hydrogen atoms in the samples: 1. Hydrogen fluoride (HF): 5.95 moles of H 2. Hydrogen sulfide (H2S): 6.98 moles of H 3. Phosphine (PH3): 10.5 moles of H 4. Water (H2O): 13.22 moles of H Thus, the samples rank from the least to the greatest number of hydrogen atoms as follows: HF < H2S < PH3 < H2O.

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Most popular questions from this chapter

In using a mass spectrometer, a chemist sees a peak at a mass of 30.0106 . Of the choices $^{12} \mathrm{C}_{2}^{1} \mathrm{H}_{6},^{12} \mathrm{C}^{1} \mathrm{H}_{2}^{16} \mathrm{O},\( and \)^{14} \mathrm{N}^{16} \mathrm{O}$ which is responsible for this peak? Pertinent masses are \(^{1} \mathrm{H}\) $1.007825 ; 16 \mathrm{O}, 15.994915 ;\( and \)^{14} \mathrm{N}, 14.003074$

A compound contains only \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{N}\) . Combustion of 35.0 \(\mathrm{mg}\) of the compound produces 33.5 $\mathrm{mg} \mathrm{CO}_{2}\( and 41.1 \)\mathrm{mg}\( \)\mathrm{H}_{2} \mathrm{O}$ . What is the empirical formula of the compound?

An iron ore sample contains \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) plus other impurities. A 752 -g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction: $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g) $$ What is the mass percent of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) in the impure iron ore sample? Assume that \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) is the only source of iron and that the reaction is 100\(\%\) efficient.

Adipic acid is an organic compound composed of 49.31\(\% \mathrm{C}\) , $43.79 \% \mathrm{O},$ and the rest hydrogen. If the molar mass of adipic acid is 146.1 \(\mathrm{g} / \mathrm{mol}\) , what are the empirical and molecular formulas for adipic acid?

Consider a mixture of potassium chloride and potassium nitrate that is 43.2\(\%\) potassium by mass. What is the percent \(\mathrm{KCl}\) by mass of the original mixture?
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