There are two naturally occurring isotopes of Copper (Cu). The table shows the two isotopes, their abundance, and their mass in amu. Calculate the average atomic mass of copper. Avg Atomic Mass = (M₁ À ) + (M‚¯A₂) ± (M₂´A,)100OR. USING DECIMAL ABUNDANCESAvg Atomic Mass = (M. A) + (M₂A₂) + (M₁A₂) Naturally Occurring Isotopes of CopperAtomic MassTatomic mass units, u)62.9364.93IsotopePercent NaturalAbundance (16)69.1730.83

Given, Relative abundance of Copper.

Answered: There are two naturally occurring…

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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There are two naturally occurring isotopes of Copper (Cu). The table shows the two isotopes, their abundance, and their mass in amu. Calculate the average atomic mass of copper.

Avg Atomic Mass = (M₁ À ) + (M‚¯A₂) ± (M₂´A,)
100
OR. USING DECIMAL ABUNDANCES
Avg Atomic Mass = (M. A) + (M₂A₂) + (M₁A₂)

Naturally Occurring Isotopes of Copper
Atomic Mass
Tatomic mass units, u)
62.93
64.93
Isotope
Percent Natural
Abundance (16)
69.17
30.83

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