3. Tungsten has 4 major isotopes. Given the atomic weight of tungsten, 183.85, complete the following table. You must show your work, avoid rounding off intermediate values, and report your % abundance values accurate to 2 decimal places. Isotope Tungsten-182 Tungsten-183 Tungsten-184 Tungsten-186 Exact Mass % Abundance 26.50 14.31 181.9482 182.9502 183.9509 185.9544

3. Tungsten has 4 major isotopes. Given the atomic weight of tungsten, 183.85, complete the following table. You must show your work, avoid rounding off intermediate values, and report your % abundance values accurate to 2 decimal places. Isotope Tungsten-182 Tungsten-183 Tungsten-184 Tungsten-186 Exact Mass % Abundance 26.50 14.31 181.9482 182.9502 183.9509 185.9544

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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2. Potassium has three naturally occurring isotopes: 3° K, 19 relative abundance =93.26% isotopic mass 38.964 amu 40K, 19 relative abundance =0.01000% isotopic mass = 39.964 amu 4'K relative abundance = 6.730% 19 isotopic mass = 40.962 amu Calculate the relative atomic mass of potassium.
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.
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
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 ? ?
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)
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46TI 48TI 71.200% 45.95263 19.900% 47.94795 50TI 8.900% 49.94479 What is the average atomic mass of titanium on that planet? u average atomic mass = TOOLS x10
Use the mass spectrum of lead shown here to estimate 100% - the atomic mass of lead. Esti- mate the mass and percent in- tensity values from the graph to three significant figures. 50%- 204 206 207 208 Mass (amu) Intensity %
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.)
An unknown element is a mixture of isotopes 151X (atomic mass= 150.99 amu) and 153X (atomic mass = 153.03 amu). The average atomic mass of X is 152.57 amu. What is the percent abundance of 153X? +
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is amu. Isotope Abundance Mass 53 X 25.00 52.62 56x 37.00 56.29 58x 38.00 58.31 Group of answer choices 55.74 57.14 56.14 55.70