Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 10

When \(3.06 \mathrm{g}\) hydrogen was allowed to react with an excess of oxygen, \(27.35 \mathrm{g}\) water was obtained. In a second experiment, a sample of water was decomposed by electrolysis, resulting in \(1.45 \mathrm{g}\) hydrogen and 11.51 g oxygen. Are these results consistent with the law of constant composition? Demonstrate why or why not.

Short Answer

Expert verified
Yes, the results are consistent with the law of constant composition. This is proven by the fact that the percentage composition of hydrogen and oxygen in water from both experiments is the same: approximately \(11.2\%\) of hydrogen and \(88.8\%\) of oxygen. This consistency in percentage composition regardless of the source or preparation of the compound is precisely what the law of constant composition states.

Step by step solution

01

Calculate the mass of oxygen in the first experiment

Firstly, calculate the mass of oxygen in the first experiment. Since hydrogen reacts with oxygen to produce water and the total mass of water is given, the mass of oxygen can be calculated as the difference between the mass of water and the mass of hydrogen. Substract \(3.06 \mathrm{g}\) (mass of hydrogen) from \(27.35 \mathrm{g}\) (mass of water) to get \(24.29 \mathrm{g}\) of oxygen.
02

Calculate the percentage of hydrogen and oxygen in the first experiment

Next, calculate the percentage composition of hydrogen and oxygen. This is done by dividing the mass of each element by the total mass of the substance, and then multiplying by 100. Here the total mass is \(27.35 \mathrm{g}\). Dividing \(3.06 \mathrm{g}\) (mass of hydrogen) by \(27.35 \mathrm{g}\), and then multiplying by 100 gives approximately \(11.2\%\). Similarly, calculating for oxygen gives approximately \(88.8\%\).
03

Calculate the percentage of hydrogen and oxygen in the second experiment

Now calculate the percentage composition of hydrogen and oxygen in the second experiment, same as in step 2. The total mass in this case is \(1.45 \mathrm{g}\) (mass of hydrogen) + \(11.51 \mathrm{g}\) (mass of oxygen) = \(12.96 \mathrm{g}\). Calculating the percentages gives approximately \(11.2\%\) for hydrogen and \(88.8\%\) for oxygen.
04

Compare the outcomes

Lastly, compare the percentage compositions from the two experiments. If they're the same for both hydrogen and oxygen (which they are in this case), this is consistent with the law of constant composition, confirming there's no violation of this law.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Iodine has many radioactive isotopes. Iodine-123 is a radioactive isotope used for obtaining images of the thyroid gland. Iodine-123 is administered to patients in the form of sodium iodide capsules that contain \(123 \mathrm{I}^{-}\) ions. Determine the number of neutrons, protons, and electrons in a single \(^{123} \mathrm{I}^{-}\) ion.

The following data on isotopic masses are from a chemical handbook. What is the ratio of each of these masses to that of\(^{12}_{6} \mathrm{c}\) ?\( \)^{17}_{35} \mathrm{CL}\( , 34.96885 \mathrm{u} ;\) (b) \(_{12}^{26} \mathrm{Mg}\) 25.98259 u ;\(^{86}_{222} \mathrm{Rn}\) , 222.0175 u.

For the atom \(^{108}\) Pd with mass 107.90389 u, determine (a) the numbers of protons, neutrons, and electrons in the atom; (b) the ratio of the mass of this atom to that of an atom of \(^{12}_{6} \mathrm{H}\)

Determine (a) the number of moles of \(\mathrm{Zn}\) in a \(415.0 \mathrm{g}\) sample of zinc metal (b) the number of \(\mathrm{Cr}\) atoms in \(147.4 \mathrm{kg}\) chromium (c) the mass of a one-trillion-atom \(\left(1.0 \times 10^{12}\right)\) sample of metallic gold (d) the mass of one fluorine atom

Refer to the periodic table inside the front cover and identify (a) the element that is in group 11 and the sixth period (b) an element with atomic number greater than 50 that has properties similar to the element with atomic number 18 (c) the group number of an element \(\mathrm{E}\) that forms an ion \(\mathrm{E}^{2-}\) (d) an element \(M\) that you would expect to form the ion \(\mathrm{M}^{3+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free