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Naturally occurring Indium has two isotopes.
4.28
%
4.28
%
of the atoms are
Indium
−
113
Indium
-
113
(
113
In
113
In
) with a mass of
112.9

u
112.9

u
and
95.72
%
95.72
%
of the atoms are
Indium
−
115
Indium
-
115
(
115
In
115
In
) with a mass of
114.9

u
114.9

u
. Calculate the average atomic mass of Indium with the correct number of significant figures.

Naturally occurring Indium has two isotopes 428 428 of the atoms are Indium 113 Indium 113 113 In 113 In with a mass of 1129 u 1129 u and 9572 9572 of the atoms class=
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Answer:

Average Molar mass is 114.8u

Explanation:

» From the formula of average Relative Atomic Mass [ RAM ]

[tex]{ \rm{RAM = \sum \frac{(isotopic \: mass \times \%abundance)}{100} }} \\ [/tex]

» We have two isotopes of Indium,

  • Indium-113, mass » 112.9u, % » 4.28%
  • Indium-115, mass » 114.9u, % » 95.72%

[tex]{ \tt{RAM = \frac{ \blue{(112.9 \times 4.28)} + { \green{(114.9 \times 95.72)}}}{100} }} \\ \\ { \tt{RAM = \frac{11481.44}{100} }} \\ \\ { \underline{ \underline{ \tt{ \: RAM = 114.8\: }}}}[/tex]

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