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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: NO鈧� (30.45%), N鈧侽鈧� (30.45%), NO (46.68%), and N鈧侽 (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 = \(\frac{14.01}{30.01}\) 脳 100 = 46.68%
03

Calculate the Mass Percentage of Nitrogen in NO鈧�

Next, we will determine the mass percentage of Nitrogen in NO鈧�. The molar mass of NO鈧� = molar mass of N + 2 脳 molar mass of O = 14.01 + 2 脳 16.00 = 46.01 g/mol Mass percentage of Nitrogen in NO鈧� = \(\frac{14.01}{46.01}\) 脳 100 = 30.45%
04

Calculate the Mass Percentage of Nitrogen in N鈧侽鈧�

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

Calculate the Mass Percentage of Nitrogen in N鈧侽

Finally, we will calculate the mass percentage of Nitrogen in N鈧侽. The molar mass of N鈧侽 = 2 脳 molar mass of N + molar mass of O = 2 脳 14.01 + 16.00 = 44.02 g/mol Mass percentage of Nitrogen in N鈧侽 = \(\frac{2 \times 14.01}{44.02}\) 脳 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. NO鈧�: 30.45% 2. N鈧侽鈧�: 30.45% 3. NO: 46.68% 4. N鈧侽: 63.62% So, the order is NO鈧�, N鈧侽鈧�, NO, and N鈧侽.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Mass Percent Composition
Mass percent composition helps us understand how much of a specific element is present in a compound compared to the entire mass of the compound. To calculate it, we need the molar mass of each element in the compound. First, add up the molar mass of all elements to find the total molar mass of the compound. Next, take the molar mass of the element of interest and divide it by the total molar mass. Multiply by 100 to convert to a percentage.

This calculation tells us the proportion of a specific element within the compound, which is crucial for understanding the nature and function of the compound.
Exploring Nitrogen Compounds
Nitrogen compounds play a significant role in various chemical processes and industries. Compounds like NO and NO鈧� are common in environmental chemistry, especially in air pollution.

N鈧侽鈧� is used in aerospace engineering, highlighting how nitrogen's versatile chemical properties can be utilized. On the other hand, N鈧侽, commonly known as laughing gas, is used in medicine.

Understanding these compounds' composition can provide insights into their chemical behavior and applications.
Decoding Chemical Formulas
Chemical formulas are shorthand notations representing the elements in a compound. For instance, NO means one nitrogen atom is bonded to one oxygen atom. In NO鈧�, one nitrogen atom is bonded to two oxygen atoms. Similarly, N鈧侽 shows two nitrogen atoms bonded with one oxygen atom, while N鈧侽鈧� displays two nitrogen atoms with four oxygen atoms.

These formulas help us quickly identify the atomic composition of a compound and are crucial for calculating properties like molar mass and mass percent composition.
Getting to Know Periodic Table Elements
The periodic table is an essential tool in chemistry that organizes elements based on their atomic number and properties. Understanding where nitrogen (N) and oxygen (O) are located helps us understand their properties.

Nitrogen, with an atomic number of 7, is a non-metal that forms strong bonds with oxygen. Oxygen, atomic number 8, is also a non-metal and highly reactive.

The periodic table gives us the molar masses needed for our calculations, making it crucial for determining the mass percent composition of compounds.

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Most popular questions from this chapter

A given sample of a xenon fluoride compound contains molecules of the type \(\mathrm{XeF}_{n}\), where \(n\) is some whole number. Given that \(9.03 \times 10^{20}\) molecules of \(\mathrm{XeF}_{n}\) weigh \(0.368 \mathrm{~g}\), determine the value for \(n\) in the formula.

Elixirs such as Alka-Seltzer use the reaction of sodium bicarbonate with citric acid in aqueous solution to produce a fizz: \(3 \mathrm{NaHCO}_{3}(a q)+\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}(a q) \longrightarrow\) $$ 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Na}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}(a q) $$ a. What mass of \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\) should be used for every \(1.0 \times 10^{2} \mathrm{mg}\) \(\mathrm{NaHCO}_{3} ?\) b. What mass of \(\mathrm{CO}_{2}(g)\) could be produced from such a mixture?

Which of the following pairs of compounds have the same empirical formula? a. acetylene, \(\mathrm{C}_{2} \mathrm{H}_{2}\), and benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}\) b. ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\), and butane, \(\mathrm{C}_{4} \mathrm{H}_{10}\) c. nitrogen dioxide, \(\mathrm{NO}_{2}\), and dinitrogen tetroxide, \(\mathrm{N}_{2} \mathrm{O}_{4}\) d. diphenyl ether, \(\mathrm{C}_{12} \mathrm{H}_{10} \mathrm{O}\), and phenol, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\)

An element \(\mathrm{X}\) forms both a dichloride \(\left(\mathrm{XCl}_{2}\right)\) and a tetrachloride \(\left(\mathrm{XCl}_{4}\right) .\) Treatment of \(10.00 \mathrm{~g} \mathrm{XCl}_{2}\) with excess chlorine forms \(12.55 \mathrm{~g} \mathrm{XCl}_{4}\). Calculate the atomic mass of \(\mathrm{X}\), and identify \(\underline{X}\)

Phosphorus can be prepared from calcium phosphate by the following reaction: \(2 \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{SiO}_{2}(s)+10 \mathrm{C}(s) \longrightarrow\) $$ 6 \mathrm{CaSiO}_{3}(s)+\mathrm{P}_{4}(s)+10 \mathrm{CO}(g) $$ Phosphorite is a mineral that contains \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) plus other nonphosphorus- containing compounds. What is the maximum amount of \(\mathrm{P}_{4}\) that can be produced from \(1.0 \mathrm{~kg}\) of phosphorite if the phorphorite sample is \(75 \% \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) by mass? Assume an excess of the other reactants.
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