   Chapter 2, Problem 23PS

Chapter
Section
Textbook Problem

Gallium has two naturally occurring isotopes, 69Ga and 71Ga, with masses of 68.9257 u and 70.9249 u, respectively. Calculate the percent abundances of these isotopes of gallium.

Interpretation Introduction

Interpretation:

The percent abundance of isotopes of Gallium has to be determined if the one isotope (69Ga) has a mass of 68.9257u and other isotope (71Ga) has a mass of 70.9249u.

Concept Introduction:

The average weight (atomic weight) of Gallium is 69.723u.

Equation for atomic weight is,

atomic weight=(%abundanceisotope-1100)×(massofisotope-1) +(%abundanceisotope-2100)×(massofisotope-2)+etc

Explanation

There are two isotopes for Gallium atom.

The mass of isotope-1 (69Ga) is 68.9257u

The mass of isotope-2 is (71Ga) is 70.9249u.

Let’s take the percent abundance of 69Ga as ‘x’ and 71Ga is ‘100-x’.

Therefore,

Equation for average weight of Gallium is,

69.723=(x100)×(68.9257)+(100-x100)×(70.9249u)69.723=(68.9257x100)+(7092.49-70.9249x100)69

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