A hypothetical element, M, with average atomic weight of 35.75. M has three stable isotopes with the masses and percentage abundances are shown below. Identify missing information on the table. % Isotopes Mass (amu) Abundance 34M 33.99 46.78 37M ? 33.93 38M 37.96 ? 3/M mass = 36.87 amu, 38M percentage abundance = 19.64%. 37M mass = 36.29 amu, 38M percentage abundance 19.89%. 3/M mass = 36.92 amu, 38M percentage abundance = 19.29%. 3/M mass = 36.92 amu, 38M percentage abundance 20.29%. 3/M mass = 32.92 amu, 38M percentage abundance 19.29%. %3D

A hypothetical element, M, with average atomic weight of 35.75. M has three stable isotopes with the masses and percentage abundances are shown below. Identify missing information on the table. % Isotopes Mass (amu) Abundance 34M 33.99 46.78 37M ? 33.93 38M 37.96 ? 3/M mass = 36.87 amu, 38M percentage abundance = 19.64%. 37M mass = 36.29 amu, 38M percentage abundance 19.89%. 3/M mass = 36.92 amu, 38M percentage abundance = 19.29%. 3/M mass = 36.92 amu, 38M percentage abundance 20.29%. 3/M mass = 32.92 amu, 38M percentage abundance 19.29%. %3D

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

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 ? ?
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
On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 71.500% 45.95263 10.500% 47.94795 Ti 18.000% 49.94479 What is the average atomic mass of titanium on that planet? Isotope 46 48 Ti Ti 50 average atomic mass= TOOLS: x10 I 11
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
On another planet, the isotopes of titanium have the given natural abundances. Mass (u) Isotope 46TI Abundance 79.400% 45.95263 48TI 11.400% 47.94795 50TI 9.200% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass = 46.69706 Incorrect
A hypothetical element, M, has four stable isotopes with the masses shown below. 109M = 108.9842 amu 107M = 106.9085 amu 105M = 104.9904 amu 103M = 102.9991 amu If the percentage abundance of 109M is 10.5%, 105M is 6.6% and the average atomic mass of M is 106.6785 amu, then what is the percentage abundance for 103M? Enter your answer as a percentage but without the % symbol. Use one decimal place.
An unknown element is a mixture of isotopes 120X and 122X. The average atomic mass of X is 121.03 amu. What is the percent abundance of 122X?
12.) Potassium (atomic mass= 39.10 amu) has three isotopes with masses 38.9367 amu, 39.9640amu, and 40. 9618 amu. The abundance of the last isotope is 6.73%. Estimate the abundances of the other two isotopes.
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.)
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
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? +