silver has two naturally occurring isotopes, one of mass 106.91 amu and the other of mass 108.90amu. FInd the fractional abundances for these two isotopes. The atomic weight is 107.87 amu

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call
Notice that the abundance of Ag-107 (106.91 amu) is assigned “x” and the Ag-109 (108.90 amu) is “1 – x”. 106.91x + 108.90(1 – x) = 107.87 106.91x + 108.90 – 108.90x = 107.87 1.99x = 1.03 x = 0.518 The fractional abundance of second isotope is 1 – 0.518 = 0.482. Answer: The fractional abundance of Ag-107 is 0.518, the fractional abundance of Ag-109 is 0.482.
0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
Gallium has two naturally occurring isotopes with mass 69 and 71 respectively. What is the peecentage abundance of both isotopes if their relative atomic mass is 70.59?

solutionLet the percentage of the isotope 71 Gallium be =y%The percentage of the isotope 69Ga is =(100−y) %Therefore, we write the mass balance equation100×69.72 = y×71+(100−y) ×696972 = 71y+6900−69y2y=6972−6900=72y=36The percentage of the isotope is =36%

1 Answers 1 views
The atomic mass of two stable isotopes of boron, 10 5B (19.78%) and 11 5B (80.22%) are 10.0129 amu and 11.0093 amu respectively. Calculate the average atomic mass of boron.

Average atomic mass=(19.78%*10.0129amu + 80.22%*11.0093amu)/100%=10.8122amu

1 Answers 1 views
boron occurs in nature in the form of two isotopes having atomic mass 10 and 11. what are the precentage abundances of two isotopes in a sample of boron haqving atomic mass 10.8

Hence the %abundance of the two isotopes are 20 80 %.

1 Answers 1 views
Potassium has two naturally occurring isotopes: k-39 ( 93.12%; mass= 38.9637 amu), and k-41 ( 6.88%; 40.9618 amu). Calculate the atomic weight for potassium.

Atomic weight for potassium=39.1011amu.

1 Answers 1 views
Natural boron is composed of two isotopes: 19.78% boron-10 (atomic mass = 10.0129 amu) and 80.22% boron-11 (atomic mass = 11.0093 amu). What is the average atomic mass of naturally occurring boron?

Average atomic mass=(19.78%*10.0129amu + 80.22%*11.0093amu)/100%=10.8122amu

1 Answers 1 views
Fictitious element X has an a average atomic mass of 254.9 and only 2 isotopes, One of its isotopes has an abundance of 72.00 and a mass of 250.9 amu. What is the atomic mass of the second isotope?

Solution:The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance.Average atomic mass = f1M1 + f2M2 +… + fnMn where...

1 Answers 1 views
What is the mass in amu of 2 molecules of Triuranium Octaoxide (U3O8)? A. 254 amu B. 208 amu C. 842 amu D. 1684 amu E. 1952 amu

The mass in amu of 2 molecules of Triuranium Octaoxide (U3O8) is 1684 (D).

1 Answers 1 views
Based on the atomic mass of the element nitrogen on the Periodic Table, compare the relative abundances of the naturally occurring isotopes of nitrogen.

The atomic mass of the element nitrogen on the Periodic Table is 14.007. It is very close to 14 - integer number. That shows that the abundance of natural isotope...

1 Answers 1 views
Calculate the nuclear binding energy per nucleon for the He nucleus. (atomic masses: He = 4.0026 amu; H = 1.0078 amu; n = 1.0087 amu; 1 amu = 1.6605 x 10-27 kg)

E= mc^2.E=1.66x10-27 x (3 x 10^8)^2=1,494e-10 kJ.

1 Answers 1 views
Element X has two naturally occurring isotopes, 10X (18.98 % abundance) and 11X (81.02 % abundance). What is the atomic mass of Element X?

We know the atomic mass= (1/100)× Σ(% abundance ×mass no.) of isotopesGiven,abundance of 10X isotope = 18.98 % Mass no. = 10abundance of 11X isotope = 81.02 %Mass no =...

1 Answers 1 views
X