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The atomic weight of a newly discovered element is 110.352 amu. It has two naturally occurring isotopes. One has a mass of 111.624 amu. The other has an isotopic mass of 109.75 amu. What is the percent abundance of the last isotope (109.75 amu)?
The idea here is that each isotope will contribute to the average of the element proportionally to their respective abundance. Now, the key to this problem lies in how you...
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Calcium has three different isotopes. One has a mass of 35.00 amu; another has a mass of 41.00 amu; and another has a mass of 40.00 amu. Which isotope is the most abundant of the three?
It follows that whatever atomic mass is quoted on the Periodic Table, the most abundant isoptope of that element must make the greatest statistical contribution. Calcium has an atomic mass...
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What is the average atomic mass of titanium if we have an isotopic distribution of $78.5%$ of $""^46Ti$, $45.95263*"amu"$, $12.3%$ of $""^48Ti$, $47.94795*"amu"$, and $""^50Ti$, $49.94479*"amu"$?
$"Atomic mass of titanium"={0.785xx45.95263+0.123xx47.94795+0.092xx49.94479}*"amu"=??$ Is this the same as on this planet?
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An average sample of chlorine contains 75.77% chlorine-35, with an atomic mass of 34.969 amu (atomic mass units), and 24.23% chlorine-37, with an atomic mass of 36.966 amu. What is the average atomic mass of chlorine?
The weighted average is the sum of each individual nuclide, multiplied by its isotopic abundance. So, we simply do the arithmetic: $0.7577xx34.969+0.2423xx36.966 = ???$ amu Then look at to...
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What is the average atomic mass of an element if, out of 100 atoms, 5 have a mass of 176 amu, 19 have a mass of 177 amu, 27 have a mass of 178 amu, 14 have a mass of 179 amu, and 35 have a mass of 180 amu?
The $"Average Atomic Mass"$ of an element is defined as "the weighted average mass of all naturally-occurring (occasionally radioactive) of the element." (and hence the name "average") [1] Dividing the...
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Magnesium has three naturally occurring isotopes with masses of 23.99 amu, 24.99 amu, and 25.98 amu and natural abundances of 78.99%, 10.00% and 11.01% respectively. How do you calculate the atomic mass of magnesium?
The is the weighted average of the individual isotopic masses: $(23.99xx78.99%+24.99xx10.00%+25.98xx11.01%)*g=24.31*g$ I have given you answer in $g$ which here is equivalent to $"amu"$.
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The mass of a hydrogen atom is 1.0 amu, and the mass of a carbon atom is 12.0 amu. What is the moiar mass of methane, $CH_4$?
Molar Mass of $CH_4= 12+4$ Molar Mass of $CH_4= 16$ amu
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How do you calculate the average atomic mass of rubidium if 72.17% of its atoms have a mass of 84.91 amu and 27.83% of its atoms have a mass of 86.91 amu?
The average of some substance is measured indeed with the percentages of how much they exist in nature. An average is always calculated by adding up the numbers and divide...
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What is the average atomic mass of an element composed of a series of isotopes, $X, Y, Z$ with respective masses, $18.473*"amu", 19.962*"amu", 21.469*"amu"$, and respective abundances, $X=28.812%$, $Y=28.757%$...?
$"Average atomic mass"={18.473_"X"xx28.812%+19.962_"Y"xx 28.757% +21.469_"Z" xx(100-28.812-28.757)%}*"amu"$ $-=20.15*"amu"$...if I have done my 'rithmetic right... How did I get the percentage abundance of $Z$? And it is likely that we got the...
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The mass of a hydrogen atom is 1.0 amu, and the mass of a carbon atom is 12.0 amu. What is the molar mass of methane?
Can you tell us the molar mass given that carbon has a molar mass of $12.0*g$, and hydrogen, $1.0*g$?
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