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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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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 atomic weight of Ga is 69.72 amu. There are only two naturally occurring isotopes of gallium: $"^69Ga$ with a weight of 69.0 amu, and $"^71Ga$ with a weight of 71.0 amu. What is approximate natural abundance of the $"^71Ga$ isotope?
Let the percentage of the isotope $""^71Ga$ be $=x%$ Then, The percentage of the isotope $""^69Ga$ is $=(100-x)%$ We write the mass balance equation $100*69.72=x*71+(100-x)*69$ $6972=71x+6900-69x$ $2x=6972-6900=72$ $x=36$ Therefore, The...
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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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How many chloride ions would combine with an $Al^(3+)$ ion to form aluminum chloride?
Al has a charge of +3. Cl has a charge of -1. Hence 3 chloride ions are required to neutralize charge of +3 on aluminium and the compound formed is...
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How can I balance this chemical equations? Potassium metal and chlorine gas combine to form potassium chloride.
let us write a chemical equation; word equation is Potassium metal + Chlorine Gas --------> Potassium Chloride The chemical equation using symbols and formula is...
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What is the equation for solid potassium chloride and oxygen gas combine to form solid potassium chlorate?
This is a synthesis reaction, also called a combination reaction in which two or more smaller reactants combine to form a single, more complex compound.
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