1 Answers
Call
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 of
0
like
0 dislike
Talk Doctor Online in Bissoy App
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...
1 Answers 1 views
Gallium has two naturally occurring isotopes. The mass of gallium-69 is 68.9256 amu and it is 60.108% abundant. The mass of gallium-71 is 70.9247 amu and it is 39.892% abundant. What is the atomic mass of gallium?
To find the average ($"A"_r$) of an element, given the percentage rarities of its , simply multiply each isotope's $"A"_r$ by its percentage that is expressed as a decimal...
1 Answers 1 views
One isotope of bromine has an atomic mass of 78.92 amu and a relative abundance of 50.69%. The other major isotope of has an atomic mass of 80.92 amu and a relative abundance of 49.31%? What is the average atomic mass of bromine?
Multiply the atomic mass of each isotope times its percent abundance in decimal form. Add them together. $"Average atomic mass of Br"$$=$$(78.92xx0.5069)+(80.92xx0.49331)="79.92 u"$
1 Answers 1 views
Argon has three naturally occurring isotopes: argon-36, argon-38, and argon-40. Based on argon's reported atomic mass, which isotope do you think is the most abundant in nature?
The mass of Argon on is 39.948. The periodic table's is the AVERAGE weight of ALL its . If one isotope is MORE abundant than the others, the average will...
1 Answers 1 views
The atomic weight of a newly discovered e ement is 98.225 amu. It has two naturally occuring isotopes. One isotope has a mass of 96.780 amu. The second isotope has a percent abundance of 41.7%. What is the mass of the second isotope?
$M_r=(sum(M_ia))/a$, where: $M_r$ = relative attomic mass ($g$ $mol^-1$) $M_i$ = mass of each isotope ($g$ $mol^-1$) $a$ = abundance, either given as a percent or amount of $g$...
1 Answers 1 views
There are 3 isotopes of carbon. Carbon-12, Carbon-13 and Carbon-14. The average atomic mass of carbon is 12.011. Which isotope of carbon is the most abundant? Why?
The relative of carbon is 12.011, which is extremely close to 12.0. This means that the masses C-13, and C-14 are practically negligible when contributing to the relative atomic mass...
1 Answers 1 views
The atomic weight of a newly discovered element is 10.600 amu. It has two naturally occurring isotopes. One has a mass of 10.000 amu
and a natural abundance of 70.000%. What
is the isotopic mass of the other isotope?
So, $10.600 (mass$ $units) = 70%xx10.000 + 30%xxM_2;$ where $M_2$ is the isoptopic mass of the other isotope. So solve for $M_2$! A priori would you expect $M_2$ to...
1 Answers 1 views
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...
1 Answers 1 views
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...
1 Answers 1 views
Isotope: 35 AMU: 34.968852 % Abundance: 75.77; Isotope: 37 AMU: 36.965903 % Abundance: 24.23
The two isotopes for Cl are chlorine-35 and chlorine-37.
What is the average mass for Cl up to 4 decimal places?
The average mass is simply the weighted average: $(34.968852xx75.77%+36.965903xx24.23%)*"amu"$ $=$ $35.4527*"amu"$
1 Answers 1 views