A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System. Mass-spectroscopic analysis produced the followin data on the isotopes of ruthenium in these samples: isotope дори mass relative (amu) abundance 95.9 44.% 104, Ru 103.9 Use these measurements to complete the entry for ruthenium in the Periodic Table that would be used on 98765 ALEKS. Round your entry for the atomic mass to 3 significant digits. e Caution: your correct answer will have the same format but not necessarily the same numbers as the entry for ruthenium in the Periodic Table we use here on Earth. 56.% Ru 0 X

A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System. Mass-spectroscopic analysis produced the followin data on the isotopes of ruthenium in these samples: isotope дори mass relative (amu) abundance 95.9 44.% 104, Ru 103.9 Use these measurements to complete the entry for ruthenium in the Periodic Table that would be used on 98765 ALEKS. Round your entry for the atomic mass to 3 significant digits. e Caution: your correct answer will have the same format but not necessarily the same numbers as the entry for ruthenium in the Periodic Table we use here on Earth. 56.% Ru 0 X

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter1: The Nature Of Chemistry

Section: Chapter Questions

Problem 118QRT

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Similar questions

The element gallium, used in gallium arsenide semiconductors, has an atomic weight of 69.72 amu. There are only two isotopes of gallium, Ga with a mass of 6.9257 amu and Ga with a mass of 70.9249 amu. What are the isotopic abundances of gallium? Gallium melts just above room temperature
An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.
Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% 6Li and 92.5% 7Li, which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% 6Li (and the rest 7Li). Calculate the average atomic mass values for each of these two sources.
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
Atomic structure. (a) The synthetic radioactive element technetium is used in many medical studies. Give the number of electrons, protons, and neutrons in an atom of technetium-99. (b) Radioactive americium-241 is used in house-hold smoke detectors and in bone mineral analysis. Give the number of electrons, protons, and neutrons in an atom of americium-241.
Verify that the atomic weight of lithium is 6.94, given the following information: 6Li, mass = 6.015121 u; percent abundance = 7.50% 7Li, mass = 7.016003 u; percent abundance = 92.50%
Calculate the atomic mass of each of the following elements using the given data for the percentage abundance and mass of each isotope. a. Lithium: 7.42% 6Li (6.01 amu) and 92.58% 7Li (7.02 amu) b. Magnesium: 78.99% 24Mg (23.99 amu), 10.00% 25Mg (24.99 amu), and 11.01% 26Mg (25.98 amu)
2. Which of the following is closest to the observed abundance of 71Ga, one of two stable gallium isotopes (69Ga and 71Ga)? 20% 60% 70% 40%