Indium has only two naturally occurring isotopes. The mass of indium-113 is 112.9041 amu and the mass of indium-115 is 114.9039 amu. Part A: Use the atomic mass of indium to calculate the relative abundance of indium-113.
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Step 1
9041 amu - Mass of indium-115 (\( m_{115} \)) = 114.9039 amu - Atomic mass of indium (\( m_{avg} \)) = 114.818 amu (this is typically found on the periodic table) Show more…
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Indium (In) has two naturally occurring isotopes: In- 113 and In- $115 .$ In- 113 has a $4.30 \%$ abundance and a mass of $112.9$ amu, and In- 115 has a $95.70 \%$ abundance and a mass of $114.9$ amu. Calculate the atomic mass for indium using the weighted average mass method. $(4.5)$
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The element indium has two stable isotopes, indium-113 with an atomic mass of 112.9 u and indium-115 with an atomic mass of 114.9 u. From the atomic weight found on the periodic table, one can conclude that: a. both isotopes have the same percent natural abundance b. there is an isotope of nitrogen with an atomic mass of 114.8 u c. indium-115 has the highest percent natural abundance d. indium-113 has the highest percent natural abundance
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