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Chapter 3: Problem 35

Use ammonia \(\left(\mathrm{NH}_{3}\right)\) to explain what is meant by the percent composition by mass of a compound.

Short Answer

Expert verified
The percent composition by mass of Nitrogen (N) and Hydrogen (H) in Ammonia are approximately 82.20% and 17.80% respectively. This is derived by dividing the atomic weight of each component by the total molecular weight of the compound and then multiplying the result by 100.

Step by step solution

01

Breakdown of Ammonia

Ammonia (NH3) consists of one Nitrogen (N) atom and three Hydrogen (H) atoms. From the periodic table, the atomic weights of Nitrogen (N) and Hydrogen (H) are approximately 14.01g/mol and 1.01g/mol respectively.
02

Calculation of Total Mass of Ammonia

Calculate the total mass of ammonia (NH3) by adding the mass of one Nitrogen atom and the masses of three Hydrogen atoms. Thus, the molar mass of NH3 = \( 14.01g/mol (for N) + 3 \times 1.01g/mol (for 3H) = 17.04g/mol \).
03

Finding the Percent Composition

The percent composition by mass of each element in a compound is calculated by dividing the total mass of each element by the total molar mass of the compound and then multiplying the result by 100. So, the percent by mass of Nitrogen (N) in ammonia (NH3) = \( \frac {14.01g/mol}{17.04g/mol} \times 100 = 82.20\% \). Similarly, the percent by mass of Hydrogen (H) in ammonia (NH3) = \( \frac {3 \times 1.01g/mol}{17.04g/mol} \times 100 = 17.80\% \).

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Most popular questions from this chapter

For many years chloroform \(\left(\mathrm{CHCl}_{3}\right)\) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that may cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of this compound.

Potash is any potassium mineral that is used for its potassium content. Most of the potash produced in the United States goes into fertilizer. The major sources of potash are potassium chloride \((\mathrm{KCl})\) and potassium sulfate \(\left(\mathrm{K}_{2} \mathrm{SO}_{4}\right)\). Potash production is often reported as the potassium oxide \(\left(\mathrm{K}_{2} \mathrm{O}\right)\) equivalent or the amount of \(\mathrm{K}_{2} \mathrm{O}\) that could be made from a given mineral. (a) If \(\mathrm{KCl}\) costs \(\$ 0.055\) per \(\mathrm{kg}\), for what price (dollar per \(\mathrm{kg}\) ) must \(\mathrm{K}_{2} \mathrm{SO}_{4}\) be sold in order to supply the same amount of potassium on a per dollar basis? (b) What mass (in \(\mathrm{kg}\) ) of \(\mathrm{K}_{2} \mathrm{O}\) contains the same number of moles of \(\mathrm{K}\) atoms as \(1.00 \mathrm{~kg}\) of \(\mathrm{KCl} ?\)

Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) is a component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air: $$ \mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} $$ (b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reagent in this reaction.

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen. $$ 3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g) $$ In a particular reaction, 6.0 moles of \(\mathrm{NH}_{3}\) were produced. How many moles of \(\mathrm{H}_{2}\) and how many moles of \(\mathrm{N}_{2}\) were reacted to produce this amount of \(\mathrm{NH}_{3} ?\)

Use the formation of water from hydrogen and oxygen to explain the following terms: chemical reaction, reactant, product.
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