A sample of lithium consists of 400 atoms. 30 atoms are the isotope Lithium-6 (6.015 amu) and 370 are Lithium-7 (7.016 amu). Which student correctly calculated the correct average atomic mass and why? Student 1 calculated the average atomic mass as 6.94 amu. Student 1 determined the percent abundance for each isotope and then multiplied the percent abundance by the average atomic mass of its isotope and took the sum. Student 2 calculated the average atomic mass as 6.52 amu. Student 2 took the average of the mass of the two isotopes of lithium. Student 3 calculated the average atomic mass as 1.06 amu. Student 3 took the sum of the average atomic masses of the isotopes and multiplied by the ratio of lithium-6 to lithium-7. Student 4 calculated the average mass as 13.0 amu. Student 4 added the mass of the two isotopes.

A sample of lithium consists of 400 atoms. 30 atoms are the isotope Lithium-6 (6.015 amu) and 370 are Lithium-7 (7.016 amu). Which student correctly calculated the correct average atomic mass and why? Student 1 calculated the average atomic mass as 6.94 amu. Student 1 determined the percent abundance for each isotope and then multiplied the percent abundance by the average atomic mass of its isotope and took the sum. Student 2 calculated the average atomic mass as 6.52 amu. Student 2 took the average of the mass of the two isotopes of lithium. Student 3 calculated the average atomic mass as 1.06 amu. Student 3 took the sum of the average atomic masses of the isotopes and multiplied by the ratio of lithium-6 to lithium-7. Student 4 calculated the average mass as 13.0 amu. Student 4 added the mass of the two isotopes.

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

Antimony has two naturally occuring isotopes, 12 Sb and 123Sb. 12'Sb has an atomic mass of 120.9038 u, and 123Sb has an atomic mass of 122.9042 u. Antimony has an average atomic mass of 121.7601 u. What is the percent natural abundance of each isotope? 121 Sb: % 123 Sb:
The element zirconium has five naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. Show your work to determine the average atomic mass. Isotope Mass % Abundance Zr-90 89.9043 51.40 Zr-91 90.9053 11.20 Zr-92 91.9046 17.10 Zr-94 93.9061 17.50 Zr-96 95.9082 2.80
Using the following data, determine the percent abundance of the third isotope and the average atomic mass of isotope X. Give as a percentage. X-22 atomic mass = 22.10498 abundance = 52.3985% X-23 atomic mass = 23.0005 abundance = 24.8731% X-24 Atomic mass = 24.0593
Chromium which has an average atomic mass of 51.9961 amu has four isotopes. The masses of its isotopes are 49.94605 amu, 51.94051 amu, 52.94065 amu and 53.93888 amu. The first two isotopes have a total abundance of 87.87% and the last isotope has an abundance of 2.365%. What is the abundance of the third isotope? Answer text
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)
Determine the mass of tin that contains 6.89×10^18 tin atom
Please do this chemistry work
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.