Question

An atom of 81^Br has an experimentally determined nuclear mass of
80.9163 amu. Calculate the mass defect, Δm, in atomic mass units
(amu).

Answer #1

The mass of a lithium?7 atom is 7.016003 amu. What is the
nuclear binding energy of a lithium?7 nucleus in units of kJ/mol
and eV/nucleus? Enter your answers in scientific notation.

a) Calculate the mass defect for U-235 which has a mass of
235.04392 amu. I got 1.865 but it's saying its wrong. b) Calculate
the nuclear binding energy per nucleon (in MeV) for U-235 which has
a mass of 235.04392 amu.

Elemental bromine, Br, has an atomic weight of 79.904 amu. There
are two stable isotopes of bromine: 79Br has a mass of 78.9183371
amu and 81Br has an atomic mass of 80.9162906 amu. Knowing that the
percent abundance of the two adds up to 100.0%, what is the percent
abundance of 81Br to three significant figures?

You know that: mass of proton (mp) = 1.007276 amu, mass of
neutron (mn) = 1.008665 amu, and mass of electron (me)= 5.485799 x
10-4 amu. Calculate the mass defect (in amu) and nuclear
binding energy (in J/nucleon) for Carbon-12 (nuclear mass:
11.996708 amu)

Calculate the mass defect in amu for Li-6 with a mass of 6.01348
amu. (Enter your answer with 5 decimal places and remember to use
the appropriate sign.)

Calculate the amount of energy produced in a nuclear reaction in
which the mass defect is 0.187456 amu.
9.3318 × 10−20 J
3.11278 × 10−28 J
1.6847 × 1016 J
2.7976 × 10−11 J

Unlike chemical reactions, for which mass is conserved, nuclear
reactions result in slight changes in mass. When mass is lost, it
becomes energy according to the equation ΔE=Δm⋅c2 where ΔE is the
energy in joules, Δm is the mass defect in kilograms, and c is the
speed of light (c=3.00×108 m/s). The mass defect is the difference
between the total mass of the products and the total mass of
reactants. The following values can be used to calculate the mass...

Calculate the quantity of energy produced per mole of U-235
(atomic mass = 235.043922 amu) for the neutron-induced fission of
U-235 to produce Te-137 (atomic mass = 136.9253 amu) and Zr-97
(atomic mass = 96.910950 amu).

Chlorine has two naturally occurring isotopes, 35Cl with an
atomic mass of 34.969 amu and 37Cl with an atomic mass of 36.966
amu. The weighted average atomic mass of chlorine is 35.45 amu.
What is the percent abundance of each isotope? Be sure your work
supports your answer.
Copper has two naturally occurring isotopes, 63Cu with an atomic
mass of 62.9296 amu and 65Cu with an atomic mass of 64.9278 amu.
The weighted average atomic mass of copper is 63.546...

A fictional element has two isotopes. Isotope 1 has a mass of
70.0 amu and a relative abundance of 80.28%.
Isotope 2 has a mass of 87.0 amu.
Find the relative abundance (%) of Isotope
Calculate the average atomic mass of the fictional element.

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