1 Answers
Call
Talk Doctor Online in Bissoy App
Atoms of oxygen-16, oxygen-17, oxygen-18 are isotopes. Compare and contrast these three isotopes.
oxygen 16 has 8 protons and 8 neutrons, oxygen 17 has 8 protons and 9 neutrons, and oxygen 18 has 8 protons and 10 neutrons.Oxygen-16 is a stable isotope of...
1 Answers 1 views
galium has 2 naturally occuring isotopes with mass number 69 and 71 reapectively what is the percentage abundance of both isotopes if their relative atomic mass equals to 70.59atomic mass unit
Percentage Abundance;Galium - 69=72%Galium - 70=28%
1 Answers 1 views
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 relative atomic mass of bromine which consists of Br 79 35 and Br 85 35 isotopes is 79.9 amu. Calculate the percent abundance of Br 79 35 and Br 85 35 in the mixture of isotopes?
Br-79 78.92?Br-81 80.92?average atomic mass=(mass% +mass% +mass%)Let y be % abundance of Br-79Let 1-y be % abundance of Br-81Br is 79. 904g/mol on the periodic table 79.904% =y+(1−y)79.904% = (78.92×y) + (80.92×(1−y))79.904% =(78.92y) +...
1 Answers 1 views
An element x has atomic number of 29has two isotopes y And Z 34 and 38 respectively.. calculate the mass number for each isotopes and the nuclear symbol.. calculate the percentage abundance
(34+29)+38-29=63+9= 72/2= 36
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
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
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
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...
1 Answers 1 views
Nitrogen is made up ot two isotopes, N-14 and N-15. Given nitrogen's atomic weight of 14.007, What is the percent abundance of each of isotopes?
Assuming atomic masses of N-14 and N-15 to be exactly 14 and 15 amu respectively,14x + 15 (1 - x) = 14.007,where x*100% is the percent abundance of N-14, and...
1 Answers 1 views