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Chapter 2: Problem 26

If the volume of a proton were similar to the volume of an electron, how will the densities of these two particles compare to each other?

Short Answer

Expert verified
The density of a proton is approximately 1836 times greater than the density of an electron, assuming their volumes are similar. This is because the mass of a proton is about 1836 times greater than that of an electron, and density is directly proportional to mass when volumes are the same.

Step by step solution

01

Finding the masses of proton and electron

The mass of a proton is approximately \(1.6726 × 10^{-27} kg\), and the mass of an electron is approximately \(9.1094 × 10^{-31} kg\).
02

Expressing the mass ratio

To compare their densities, we need to find the ratio of their masses, which can be expressed as: \[ \frac{mass_{proton}}{mass_{electron}} = \frac{1.6726 × 10^{-27} kg}{9.1094 × 10^{-31} kg} \]
03

Calculate the mass ratio

Now, let's calculate the mass ratio: \[ \frac{1.6726 × 10^{-27} kg}{9.1094 × 10^{-31} kg} \approx 1836 \]
04

Comparing densities

Since the volumes of the proton and electron are assumed to be similar, the ratio of their masses will be the same as the ratio of their densities. Therefore, the density of a proton is approximately 1836 times greater than the density of an electron.

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Most popular questions from this chapter

Name the compounds in parts a–d and write the formulas for the compounds in parts e–h. a. \(\mathrm{Hg}_{2} \mathrm{O}\) b. \(\mathrm{FeBr}_{3}\) c. \(\mathrm{CoS}\) d. \(\mathrm{TiCl}_{4}\) e. tin(II) nitride f. cobalt(III) iodide g. mercury(II) oxide h. chromium(VI) sulfide

Which of the following is(are) correct? a. \(^{40} \mathrm{Ca}^{2+}\) contains 20 protons and 18 electrons. b. Rutherford created the cathode-ray tube and was the founder of the charge- to-mass ratio of an electron. c. An electron is heavier than a proton. d. The nucleus contains protons, neutrons, and electrons

A single molecule has a mass of \(7.31 \times 10^{-23}\) g. Provide an example of a real molecule that can have this mass. Assume the elements that make up the molecule are made of light isotopes where the number of protons equals the number of neutrons in the nucleus of each element.

Early tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium. How do your values compare with those in the periodic table? How do you account for any differences?

Observations of the reaction between nitrogen gas and hydrogen gas show us that 1 volume of nitrogen reacts with 3 volumes of hydrogen to make 2 volumes of gaseous product, as shown below: Determine the formula of the product and justify your answer.
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