2. Calculate the average atomic mass of Element Sh. Sh has three isotopes: 39Sh, 40Sh, and 41Sh. 39Sh has an atomic mass of 39.002 amu and occurs at an abundance of 83.25%. 40Sh has an atomic mass of 39.995 amu and occurs at an abundance of 0.049%. 41Sh has an atomic mass of 40.896 amu and occurs at an abundance of 16.701%. Show your work.

2. Calculate the average atomic mass of Element Sh. Sh has three isotopes: 39Sh, 40Sh, and 41Sh. 39Sh has an atomic mass of 39.002 amu and occurs at an abundance of 83.25%. 40Sh has an atomic mass of 39.995 amu and occurs at an abundance of 0.049%. 41Sh has an atomic mass of 40.896 amu and occurs at an abundance of 16.701%. Show your work.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 6.167 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 10.27 grams of Co, and 3.365 grams of H20 are produced. In a separate experiment, the molar mass is found to be 132.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H, O empirical formula = molecular formula =
On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 70.200% 45.95263 15.000% 47.94795 14.800% 49.94479 Isotope 46 Ti 48 Ti 50 Ti What is the average atomic mass of titanium on that planet? average atomic mass= 12.4687 Incorrect
Silicon (average atomic mass=28.0855amu) has three isotopes. Their masses are 27.9769amu, 28.9765amu, and 29.9738amu. The abundance of the heaviest isotope is 2.96%. Estimate the abundances of the first two isotopes.
On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 74.200% 45.95263 15.100% 47.94795 10.700% 49.94479 Isotope 46 Ti 48 Ti 50 Ti What is the average atomic mass of titanium on that planet? average atomic mass= x10 TOOLS u
Abundance = 74.200%, Mass(u) = 45.95263 Abundance = 14.500%, Mass = 47.94795 Abundance = 11.300%, Mass = 49.94479 average atomic mass = ??? Isotopes Ti 46, Ti 48, Ti 50
On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) Isotope 46Tİ 73.100% 45.95263 48Ti 19.500% 47.94795 50TI 7.400% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass = * TOOLS х10
A new element is discovered and has three stable isotopes. The atomic weight of the element is 269.7374 amu. Isotope X-268 has a measured mass of 267.9086 amu and an abundance of exactly 0.2 (infinite sig figs) Isotope X-272 has a measured mass of 271.8937 amu and an abundance of exactly 0.45 (infinite sig figs) What is the mass (in amu) of the other isotope? Report to the ten thousands place (4 decimal places)
A 11.90 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 16.87 grams of Co, and 10.36 grams of H20 are produced. In a separate experiment, the molar mass is found to be 62.07 g/mol. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H, O empirical formula = molecular formula =
On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 77.200% 45.95263 10.400% 47.94795 12.400% 49.94479 Isotope 46 Ti 48 Ti 50 Ti What is the average atomic mass of titanium on that planet? average atomic mass= u
Antimony has 2 stable isotopes 121-Sb mass 120.9038 and 123-Sb mass 122.9042 amu. Calculate the percent abundances of these isotopes.
6) Complete the following table by calculating the atomic mass. Isotope Mass of Atom (u) Percent Abundance (%) ¹H 2H 12C 13C 160 170 180 1.007825 2.1040 12.0 13.003355 15.994915 16.999131 17.999160 99.985 0.015 98.90 1.10 99.762 0.038 0.200 Atomic Mass (u)
3) Calculate the atomic mass of the following element with three isotopes (masses and relative abundances given below). Referring to the periodic table, identify the element. 27.9769 u, 92.2232% 28.9765 u, 4.6858% 29.9738 u, 3.0921%