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Brilliant_brown [7]
3 years ago
9

What is the atomic mass of bromine, given the atomic masses and percent abundance of the two isotopes are 78.92 amu (50.7%) and

80.92 amu (49.3%)?
Select one:
a. 79.9 amu
b. 78.9 amu
c. 80.9 amu
d. 35 amu
Chemistry
1 answer:
mojhsa [17]3 years ago
6 0

Answer:

79.9 amu

Explanation:

Given data:

Atomic mass of bromine = ?

Percent abundance of 1st isotope = 50.7%

Atomic mass of 1st isotope = 78.92 amu

Percent abundance of 2nd isotope = 49.3%

Atomic mass of 2nd isotope =80.92 amu

Solution:

Average atomic mass  = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass)  / 100

Average atomic mass = (50.7×78.92)+(49.3×80.92) /100

Average atomic mass =  4001.24 + 3989.36 / 100

Average atomic mass = 7990.6 / 100

Average atomic mass = 79.9 amu.

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c. rate=−1/2Δ[HBr]/Δt=Δ[H2]/Δt=Δ[Br2]/Δt

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

2HBr(g)\rightarrow H_2(g)+Br_2(g)

Thus, the rate is given as:

rate=-\frac{1}{2} \frac{\Delta [HBr]}{\Delta t}=\frac{\Delta [Br_2]}{\Delta t} =\frac{\Delta [H_2]}{\Delta t}

It is necessary to remember that each concentration to time interval is divided into the stoichiometric coefficient, that is why HBr has a 1/2. Moreover, the concentration HBr is negative since it is a reactant and it has a negative rate due to its consumption.

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