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Chapter 2: Problem 19

When hydrogen is burned in oxygen to form water, the composition of water formed does not depend on the amount of oxygen reacted. Interpret this in terms of the law of definite proportion.

Short Answer

Expert verified
The composition of water formed from the reaction of hydrogen and oxygen does not depend on the amount of oxygen reacted, which adheres to the law of definite proportions. This law states that a chemical compound always contains its component elements in a fixed ratio by mass. In this case, the balanced chemical equation (2H2 + O2 鈫� 2H2O) shows a 2:1 ratio of hydrogen to oxygen in water by molecule, and a 1:1 ratio by mass, confirming that water has a fixed composition according to the law of definite proportions.

Step by step solution

01

Identify the elements involved in the reaction.

In the given reaction, hydrogen (H) is burned in oxygen (O) to form water (H2O).
02

Write down the balanced chemical equation for the reaction.

To balance the chemical equation, we must ensure that the same number of each type of atom is present on both sides of the equation. The balanced chemical equation for the reaction is: \[2H_2 + O_2 \rightarrow 2H_2O\]
03

Observe the ratio of elements in the balanced equation.

In the balanced chemical equation, we see that two molecules of hydrogen react with one molecule of oxygen to form two molecules of water. Thus, the ratio of hydrogen to oxygen in the water is always 2:1 by molecule. This means there are two hydrogen atoms for every oxygen atom in a water molecule.
04

Interpret the given information in terms of the law of definite proportions.

The fact that the composition of water does not change, regardless of the amount of oxygen reacted, adheres to the law of definite proportions. No matter how much oxygen we use in the reaction, the ratio of hydrogen to oxygen in the resulting water will always be 2:1 by molecule (or 1:1 by mass, since hydrogen has approximately half the atomic mass of oxygen). This shows that water is a chemical compound with a fixed composition by mass, confirming the law of definite proportions.

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Most popular questions from this chapter

You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: \(30.43 \% \mathrm{X}, 69.57 \% \mathrm{Y}\) Compound \(\mathrm{II} : 63.64 \% \mathrm{X}, 36.36 \% \mathrm{Y}\) In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react 鈥済as X鈥� with 鈥済as Y鈥� to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas \(\mathrm{X}^{\prime \prime}+2\) volumes "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound I 2 volumes \(^{4}\) gas \(\mathrm{X}^{\prime \prime}+1\) volume "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.

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Section 2.3 describes the postulates of Dalton鈥檚 atomic theory. With some modifications, these postulates hold up very well regarding how we view elements, compounds, and chemical reactions today. Answer the following questions concerning Dalton鈥檚 atomic theory and the modifications made today. a. The atom can be broken down into smaller parts. What are the smaller parts? b. How are atoms of hydrogen identical to each other, and how can they be different from each other? c. How are atoms of hydrogen different from atoms of helium? How can H atoms be similar to He atoms? d. How is water different from hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\)even though both compounds are composed of only hydrogen and oxygen? e. What happens in a chemical reaction, and why is mass conserved in a chemical reaction?

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