29 Naturally occurring silicon consists of 20Si (27.9769 amu), 2Si (28.9765 amu) and 30 Si (29.9738 amu). The natural abundance of Si is 4.67%. If a precise periodic table shows 28.0855 amu for silicon, what are the natural abundances of 28 Si and 30 Si? a) 47.67% 28Si and 47.67% 30 Si b) 68.47% 28Si and 26.85% 30 Si c) 92.23% 2Si and 3.10% 30 Si d) 93.71% Si and 1.62% 30 Si

29 Naturally occurring silicon consists of 20Si (27.9769 amu), 2Si (28.9765 amu) and 30 Si (29.9738 amu). The natural abundance of Si is 4.67%. If a precise periodic table shows 28.0855 amu for silicon, what are the natural abundances of 28 Si and 30 Si? a) 47.67% 28Si and 47.67% 30 Si b) 68.47% 28Si and 26.85% 30 Si c) 92.23% 2Si and 3.10% 30 Si d) 93.71% Si and 1.62% 30 Si

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...

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The element lead consists of four naturally occurring isotopes with atomic masses 203.97302, 205.97444, 206.97587 and 207.97663 u. The relative abundance of these four isotopes are 1.400, 24.10, 22.10 and 52.40 % respectively. From these data, calculate the atomic weight of lead.
3) Atmospheric argon is a mixture of three stable isotopes 36Ar, 38Ar, and 40Ar. Use the information below to determine the atomic mass and natural abundance of 40Ar. The atomic weight of argon is 39.948 u. Argon-36 35.967545 u 0.337% Argon-38 37.96732 u 0.063% Argon-40 ? ?
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A certain element has five stable isotopes with the following masses and percent abundance: Isotope 1: 63.929147 amu, 48.63% Isotope 2: 65.926037 amu, 27.90% Isotope 3: 66.927131 amu, 4.100% Isotope 4: 67.924848 amu, 18.75% Isotope 5: 69.925325 amu, 0.6200% What is the atomic mass of this element? (Do not round intermediate calculations.)
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%