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Chapter 2: Problem 12

Sodium reacts with oxygen in air to form two compounds: sodium oxide and sodium peroxide. In forming sodium oxide, \(23.0 \mathrm{~g}\) of sodium combines with \(8.0 \mathrm{~g}\) of hydrogen. In forming sodium peroxide, \(23.0 \mathrm{~g}\) of sodium combines with \(16.0 \mathrm{~g}\) of oxygen. (a) What are the mass ratios of oxygen in the two compounds? (b) What fundamental law does this experiment demonstrate?

Short Answer

Expert verified
a) The mass ratios of oxygen in sodium oxide and sodium peroxide are \(\frac{8}{31}\) and \(\frac{16}{39}\), respectively. b) The fundamental law this experiment demonstrates is the Law of Multiple Proportions.

Step by step solution

01

Mass ratio of oxygen in sodium oxide

We are given that the mass of sodium is \(23.0 \mathrm{~g}\) and the mass of oxygen is \(8.0\mathrm{~g}\). The mass ratio of oxygen in sodium oxide is calculated as follows: Mass Ratio of Oxygen in Sodium Oxide (NaO) = \(\frac{\text{Mass of Oxygen}}{\text{Mass of Sodium + Mass of Oxygen}}\) Mass Ratio of Oxygen (NaO) = \(\frac{8}{23 + 8}\) = \(\frac{8}{31}\)
02

Mass ratio of oxygen in sodium peroxide

Similarly, the mass of sodium is \(23.0 \mathrm{~g}\) and the mass of oxygen is \(16.0\mathrm{~g}\). The mass ratio of oxygen in sodium peroxide is calculated as follows: Mass Ratio of Oxygen in Sodium Peroxide (NaO2) = \(\frac{\text{Mass of Oxygen}}{\text{Mass of Sodium + Mass of Oxygen}}\) Mass Ratio of Oxygen (NaO2) = \(\frac{16}{23 + 16}\) = \(\frac{16}{39}\) Thus, the mass ratios of oxygen in sodium oxide and sodium peroxide are \(\frac{8}{31}\) and \(\frac{16}{39}\), respectively. Step 2: Identify the fundamental law this experiment demonstrates
03

Fundamental law demonstrated

The mass ratios of oxygen in the two compounds of sodium show that the mass of oxygen that combines with a fixed mass of sodium is in a simple whole number ratio (1:2). This experiment demonstrates the fundamental law known as the Law of Multiple Proportions. In summary, a) The mass ratios of oxygen in sodium oxide and sodium peroxide are \(\frac{8}{31}\) and \(\frac{16}{39}\), respectively. b) The fundamental law this experiment demonstrates is the Law of Multiple Proportions.

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Key Concepts

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

Chemical Reactions
Chemical reactions are processes where substances known as reactants transform into new substances called products. In the context of sodium compounds reacting with oxygen, sodium undergoes a chemical change to form different types of oxide. This involves breaking bonds in the sodium and oxygen molecules, and forming new bonds in sodium oxide and sodium peroxide. Each compound has distinct properties, reflecting the new chemical structures formed.
Sodium oxide and sodium peroxide form as products, showcasing how the same element can react in different ways under diverse conditions. Here, the difference lies in the amount of oxygen that combines with sodium, leading to two distinct chemical reactions.
Understanding chemical reactions helps explain how elements interact to form a wide variety of compounds, which is a foundation of chemistry.
Mass Ratios
Mass ratios in a compound express the proportion of each element in the compound in terms of mass. They are fundamental in understanding the composition of compounds. For sodium oxide and sodium peroxide, the ratios of oxygen to sodium are \(\frac{8}{31}\) and \(\frac{16}{39}\), respectively.
These ratios reveal how much of oxygen combines with a fixed amount of sodium.
This helps us understand the different ways sodium and oxygen can combine to form various compounds.
The mass ratio is calculated by taking the mass of an element and dividing it by the total mass of the compound. These ratios often help in identifying laws like the Law of Multiple Proportions, where elements combine in simple whole number ratios.
Sodium Compounds
Sodium compounds are chemical compounds containing the element sodium, well-known for its reactivity and presence in many forms around us. The two sodium compounds discussed in this context are sodium oxide (\(\text{Na}_2\text{O}\)) and sodium peroxide (\(\text{Na}_2\text{O}_2\)).
Each compound has unique chemical and physical properties since they contain different amounts of oxygen in their formula. Sodium oxide is usually formed when sodium burns in a limited supply of oxygen, producing a white powder useful in ceramics and the glass industry. Sodium peroxide, containing more oxygen, is produced under more abundant oxygen conditions and is often used as a bleaching agent and in oxygen generation.
Sodium's versatility in forming various compounds highlights the vast array of chemical reactions possible with even a single element.

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Most popular questions from this chapter

Chloropropane is derived from propane by substituting Cl for \(\mathrm{H}\) on one of the carbon atoms. (a) Draw the structural formulas for the two isomers of chloropropane. (b) Suggest names for these two compounds.

Suppose a scientist repeats the Millikan oil-drop experiment but reports the charges on the drops using an unusual (and imaginary) unit called the warmomb (wa). The scientist obtains the following data for four of the drops: $$ \begin{array}{lc} \hline \text { Droplet } & \text { Calculated Charge (wa) } \\ \hline \text { A } & 3.84 \times 10^{-8} \\ \text {B } & 4.80 \times 10^{-8} \\ \text {C } & 2.88 \times 10^{-8} \\ \text {D } & 8.64 \times 10^{-8} \\ \hline \end{array} $$ (a) If all the droplets were the same size, which would fall most slowly through the apparatus? (b) From these data, what is the best choice for the charge of the electron in warmombs? (c) Based on your answer to part (b), how many electrons are there on each of the droplets? (d) What is the conversion factor between warmombs and coulombs?

Millikan determined the charge on the electron by studying the static charges on oil drops falling in an electric field (Figure 2.5\()\). A student carried out this experiment using several oil drops for her measurements and calculated the charges on the drops. She obtained the following data: $$ \begin{array}{lc} \hline \text { Droplet } & \text { Calculated Charge (C) } \\ \hline \text { A } & 1.60 \times 10^{-19} \\ \text {B } & 3.15 \times 10^{-19} \\ \text {C } & 4.81 \times 10^{-19} \\ \text {D } & 6.31 \times 10^{-19} \\ \hline \end{array} $$ (a) What is the significance of the fact that the droplets carried different charges? (b) What conclusion can the student draw from these data regarding the charge of the electron? (c) What value (and to how many significant figures) should she report for the electronic charge?

Two substances have the same molecular and empirical formulas. Does this mean that they must be the same compound?

For each of the following elements, write its chemical symbol, locate it in the periodic table, give its atomic number, and indicate whether it is a metal, metalloid, or nonmetal: (a) radon, (b) tellurium, (c) cadmium, (d) chromium, (e) barium, (f) selenium, \((\mathbf{g})\) sulphur.
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