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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
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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 %.
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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.
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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
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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...
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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...
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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).
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Boron is composed of two isotopes, 10B (10.013 u) and 11B (11.009 u). If the average
atomic mass of Boron is 10.81 u, calculate the percentage abundance of 10B and 11B.
At first we may designate percentage as parts of 1: B10 content as x and B11 content as y. If there are only two isotopes, so their sum will be...
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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.
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What percentage of the mass of the isotope boron-10 do its neutrons contribute? proton = 1.0073 amu neutron = 1.0087 amu electron = 5.4858×10<sup>-4</sup> amu ............%
5 neutron 5 protons and 5 electrons.neutron = 5×1.0087 = 5.0435total = 5×1.0073 + 5×1.0087 + 5×5.4858x10-4total = 5.0365 + 5.0435 + 0.0027429total = 10.0827429percentage of neutron = (neutron/total )x100=[...
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