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Chapter 3: Problem 69

Several important compounds contain only nitrogen and oxygen. Place the following compounds in order of increasing mass percent of nitrogen. a. NO, a gas formed by the reaction of \(\mathrm{N}_{2}\) with \(\mathrm{O}_{2}\) in internal combustion engines b. \(\mathrm{NO}_{2}\), a brown gas mainly responsible for the brownish color of photochemical smog c. \(\mathrm{N}_{2} \mathrm{O}_{4}\), a colorless liquid used as fuel in space shuttles d. \(\mathrm{N}_{2} \mathrm{O}\), a colorless gas sometimes used as an anesthetic by dentists (known as laughing gas)

Short Answer

Expert verified
The order of the compounds based on increasing mass percent of nitrogen is: NO₂ (30.45%), N₂O₄ (30.45%), NO (46.68%), and N₂O (63.62%).

Step by step solution

01

Determine the Molar Mass of Nitrogen and Oxygen

The first step is to determine the molar mass of nitrogen (N) and oxygen (O). Using the periodic table, we get the following values: Molar mass of Nitrogen (N) = 14.01 g/mol Molar mass of Oxygen (O) = 16.00 g/mol
02

Calculate the Mass Percentage of Nitrogen in NO

Now we will calculate the mass percentage of nitrogen in NO. The molar mass of NO = molar mass of N + molar mass of O = 14.01 + 16.00 = 30.01 g/mol Mass percentage of Nitrogen in NO = \(\frac{14.01}{30.01}\) × 100 = 46.68%
03

Calculate the Mass Percentage of Nitrogen in NO₂

Next, we will determine the mass percentage of Nitrogen in NO₂. The molar mass of NO₂ = molar mass of N + 2 × molar mass of O = 14.01 + 2 × 16.00 = 46.01 g/mol Mass percentage of Nitrogen in NO₂ = \(\frac{14.01}{46.01}\) × 100 = 30.45%
04

Calculate the Mass Percentage of Nitrogen in N₂O₄

Now, let's find the mass percentage of Nitrogen in N₂O₄. The molar mass of N₂O₄ = 2 × molar mass of N + 4 × molar mass of O = 2 × 14.01 + 4 × 16.00 = 92.02 g/mol Mass percentage of Nitrogen in N₂O₄ = \(\frac{2 \times 14.01}{92.02}\) × 100 = 30.45%
05

Calculate the Mass Percentage of Nitrogen in N₂O

Finally, we will calculate the mass percentage of Nitrogen in N₂O. The molar mass of N₂O = 2 × molar mass of N + molar mass of O = 2 × 14.01 + 16.00 = 44.02 g/mol Mass percentage of Nitrogen in N₂O = \(\frac{2 \times 14.01}{44.02}\) × 100 = 63.62%
06

Arrange the Compounds in Order of Increasing Mass Percent of Nitrogen

Now we will arrange the compounds in order of increasing mass percentage of nitrogen: 1. NO₂: 30.45% 2. N₂O₄: 30.45% 3. NO: 46.68% 4. N₂O: 63.62% So, the order is NO₂, N₂O₄, NO, and N₂O.

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Most popular questions from this chapter

The empirical formula of styrene is \(\mathrm{CH}\); the molar mass of styrene is \(104.14 \mathrm{~g} / \mathrm{mol}\). What number of \(\mathrm{H}\) atoms are present in a \(2.00-\mathrm{g}\) sample of styrene?

Consider the following unbalanced equation: \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{CaSO}_{4}(s)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q)\) What masses of calcium sulfate and phosphoric acid can be produced from the reaction of \(1.0 \mathrm{~kg}\) calcium phosphate with \(1.0\) \(\mathrm{kg}\) concentrated sulfuric acid \(\left(98 \% \mathrm{H}_{2} \mathrm{SO}_{4}\right.\) by \(\left.\mathrm{mass}\right)\) ?

A substance \(\mathrm{X}_{2} Z\) has the composition (by mass) of \(40.0 \% \mathrm{X}\) and \(60.0 \% \mathrm{Z}\). What is the composition (by mass) of the compound \(\mathrm{XZ}_{2}\) ?

Calculate the percent composition by mass of the following compounds that are important starting materials for synthetic polymers: a. \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{2}\) (acrylic acid, from which acrylic plastics are made) b. \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\) (methyl acrylate, from which Plexiglas is made) c. \(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}\) (acrylonitrile, from which Orlon is made)

Vitamin A has a molar mass of \(286.4 \mathrm{~g} / \mathrm{mol}\) and a general molecular formula of \(\mathrm{C}_{x} \mathrm{H}_{\mathrm{y}} \mathrm{E}\), where \(\mathrm{E}\) is an unknown element. If vitamin \(\mathrm{A}\) is \(83.86 \% \mathrm{C}\) and \(10.56 \% \mathrm{H}\) by mass, what is the molecular formula of vitamin \(\mathrm{A}\) ?
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