If bromine atom is available in the form of, say, two isotopes
79br (49.7%) and 81 br (50.3%). calculate the average atomic
mass of bromine atom.

Answers

The average atomic mass of an element can be determined by multiplying the individual masses of the isotopes with their respective relative abundances, and adding them. 

Average atomic mass of Br = 158 amu(0.2569) + 160 amu(0.4999) + 162 amu(0.2431)
Average atomic mass = 159.96 amu

As described in the problem, the relative abundance for Br-79 is 25.69%. This is because 2 atoms of Br is equal to 79*2 = 158 amu. Similarly, the relative abundance of Br-81 is 81*2 = 162, which is 24.31%.
Average atomic mass of carbon is 12.01 amu

ur answer i would beileve is a

The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance (the decimal associated with percent of atoms of that element that are of a given isotope).

Average atomic mass = f1M1 + f2M2 +… + fnMn where f is the fraction representing the natural abundance of the isotope and M is the mass number (weight) of the isotope.

Explanation:

Explanation: wsp

how ur day

Answer is: the average atomic mass of 125 atoms of uranium is 235.88.

ω(U-234) = 10 ÷ 125.

ω(U-234) = 0.080.

ω(U-235) = 75 ÷ 125.

ω(U-235) = 0.60.

ω(U-238) = 40 ÷ 125.

ω(U-238) = 0.320.

Average atomic mass of atoms of uranium =

Ar(U-234) · ω(U-234) + Ar(U-235) · ω(U-235) + Ar(U-238) · ω(U-238).

Average atomic mass of atoms of uranium =

234 · 0.08 + 235 · 0.6 + 238 · 0.32.

Average atomic mass of atoms of uranium = 18.72 + 141 + 76.16.

Average atomic mass of atoms of uranium = 235.88.

Answer in explanation

Explanation:

The atomic mass can be defined as the addition of the number of protons and neutrons in the nucleus of an atom. When we talk of atomic mass, we are considering the mass of a particular isotope.

The average atomic mass or otherwise called the relative atomic mass is the atomic mass of the element itself. It has been calculated by taking into consideration the atomic masses of all the contributing isotopes existing in nature.

For example we have carbon 14 and carbon 12. While 14 is the atomic mass of that isotope, 12 is the relative atomic mass of the carbon atom. The abundance in nature of the different isotopes will dictate where the final atomic mass will lean

A) 35.45 amu

Explanation:

Average molar mass is given as

M_{avg} = \frac{n_1M_1 + n_2M_2}{n_1 + n_2}

here we know that

n_1 = 0.75

M_1 = 35

n_2 = 0.25

M_2 = 37

now we have

M_{avg} = \frac{0.75(35) + 0.25(37)}{0.75 + 0.25}

M_{avg} = 35.5

(75% of  35)  + (25% of 37)

0.75*35  + 0.25*37 = 35.5

35.50 amu  

80 amu

Explanation:

Data Given:

Abundance of Br-79 = 49.7 % = 0.497

mass of Br-79 = 79 amu

Abundance of Br-81 = 50.3% = 0.503

mass of Br-81 = 81 amu

Average atomic mass of bromine atom = ?

Solution:

Formula used to check average atomic mass is as under

                      Average atomic mass = m₁A₁ + m₂A₂

Where

m₁ and m₂ = mass of isotope 1 and 2 respectively

A₁ and A₂ = abundance or fraction of isotope 1 and 2 respectively

Put values in above formula

            Average atomic mass = (79 amu)(0.497) + (81 amu)(0.503)

            Average atomic mass = 39.263 + 40.743

            Average atomic mass = 80.006 amu

So

Round to four significant figures

Average atomic mass of Br atom= 80 amu



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