Calculating Approximate Atomic Mass of Lead | Isotopes of Pb and Percent by Mass

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Discussion Overview

The discussion revolves around calculating the approximate atomic mass of lead (Pb) using its isotopes and their percent by mass. Participants explore the reasons why the calculated atomic mass is only an approximation, touching on concepts related to isotopic composition and atomic mass versus mass number.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Debate/contested

Main Points Raised

  • One participant presents a calculation of the approximate atomic mass of lead based on given isotopes and their percent by mass.
  • Another participant questions the validity of the calculated atomic mass, suggesting that the sum of the percentages should equal 100% and pointing out a potential error in the conversion of percentages.
  • Some participants express confusion about why the calculated atomic mass is only approximate, with suggestions that it may be due to not accounting for all isotopes or the mass of electrons.
  • There is a discussion about the difference between mass numbers and atomic masses, with a participant emphasizing the need to use atomic masses for accurate calculations.
  • Participants mention that the remaining 0.01% of isotopes could contribute to the approximation error, indicating uncertainty about the complete isotopic composition of lead.
  • Clarifications are made regarding the atomic mass of specific isotopes, with references to external sources for accurate values.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the exact reasons for the approximation of the atomic mass. While some agree that the calculation does not account for all isotopes, others suggest that the confusion lies in the distinction between mass numbers and atomic masses.

Contextual Notes

Participants express uncertainty about the exact atomic masses of isotopes and the implications of using mass numbers instead of atomic masses in calculations. There are unresolved questions regarding the isotopic composition of lead and how it affects the accuracy of the calculated atomic mass.

tigerwoods99
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Homework Statement


1. The Table below lists the isotopes of Pb and their percent by mass:

Isotope

% Mass

82p, 122n 1.37%

82p, 124n 26.25%

82p, 125n 20.82%

82p, 126n 51.55%(a) Using these data, calculate the approximate atomic mass of lead;

(b) Why is this number in (a) only approximate?

Show all work!

Homework Equations



Look below, i was able to solve A, however I am wondering why this number is only an approximate? Thanks!

The Attempt at a Solution



82p, 122n --> 204 mass number (.1370)
82p, 124n --> 206 mass number (.2625)
82p, 125n --> 207 mass number (.2082)
82p, 126n --> 208 mass number (.5155)

(204*.1370) + (206*.2625) + (207*.2082) + (208*.5155) = approximate atomic mass of lead
(27.95) + (54.08) + (43.10) + (107.2) = approximate atomic mass of lead
(a) 232.3 amu = approximate atomic mass of lead
 
Last edited:
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100.00%?

No need for crying, we can read standard font no problems.
 
Borek said:
100.00%?

No need for crying, we can read standard font no problems.


Im just trying to figure out the answer to the part that says like why is the average weight using the % natural occurrence only an approximate.
 
And I have gave you a hint. Do you know 100.00% composition of the mixture?
 
Borek said:
And I have gave you a hint. Do you know 100.00% composition of the mixture?

im not sure, not really understanding what you are talking about
 
tigerwoods99 said:

Homework Statement


The Attempt at a Solution



82p, 122n --> 204 mass number (.1370)
82p, 124n --> 206 mass number (.2625)
82p, 125n --> 207 mass number (.2082)
82p, 126n --> 208 mass number (.5155)

(204*.1370) + (206*.2625) + (207*.2082) + (208*.5155) = approximate atomic mass of lead
(27.95) + (54.08) + (43.10) + (107.2) = approximate atomic mass of lead
(a) 232.3 amu = approximate atomic mass of lead

Somewhere this is wrong, If you have all the individual masses in the range 204-208, how can the average be 232?

As to why it's approximate, what is the relative atomic mass of 204Pb?
 
You have assumed that fractions given sum to 100%, but have you checked it?

What if I will tell you that lead contains 26.25% of ^{124}_{82}Pb and 20.82% ^{125}_{82}Pb? Will you be able to calculate average atoms mass?

Edit: sjb is right, I missed something important :blushing:
 
Ok yea i found my error, I converted 1.37% to .1370 instead of .0137. So the approximate atomic mass of lead would be 207.1912.

I'm still confused on why this number is an approximate.
 
That sounds better, yes. What is the relative atomic mass of 204Pb?
 
  • #10
sjb-2812 said:
that sounds better, yes. What is the relative atomic mass of 204pb?

204?
 
  • #11
No. Less than that.
 
  • #12
I'm not sure... it says 204.

http://www.wolframalpha.com/entities/isotopes/lead_204/2y/re/x8/
 
Last edited by a moderator:
  • #13
tigerwoods99 said:
I'm not sure... it says 204.

http://www.wolframalpha.com/entities/isotopes/lead_204/2y/re/x8/

No. Read again. You are not looking for a mass number.
 
Last edited by a moderator:
  • #14
82 ?
 
  • #15
What are you calculating?
 
  • #16
is it 204*0.0137? = 2.7948 ?? I'm not really sure what you asking me to do.
 
  • #17
You are calculating AVERAGE ATOMIC MASS, so to get correct result you should use ATOMIC MASSES, not mass numbers.
 
  • #18
Ok, So i got that 207.1912 is the approximate atomic mass of lead. Now i just need to figure out why this number is only an approximate.
 
  • #19
Previous one was approximate, this one (assuming you took atomic masses for all isotopes) should be correct. That is, you have no idea what is 0.01% of the mixture, so there is still some error in calculations.
 
  • #20
Ok so this was my starting data
82p, 122n 1.37%

82p, 124n 26.25%

82p, 125n 20.82%

82p, 126n 51.55%

So the reason this calculation is an approximate is because the atomic mass did not take into consideration the electrons, is that correct? Or why is it an approximate, even with the atomic masses. B/c i know atomic mass = protons + neutrons but the electrons are very minute
 
  • #21
No, I think the RAM takes into account electrons. What does the Wolfram page you have quoted say is the atomic mass of lead-204?
 
  • #23
Alright, but I am still not sure where I am headed with this. I got the right number correct? It's just a matter of explaining why this number is only an approximate.

Thanks everyone
 
  • #24
Question is confusing, that's not your fault.

If you use 204 for atomic mass of the ^{122}_{82}Pb your result will be off for obvious reason - atomic mass of ^{122}_{82}Pb is NOT 204. But if you will use 203.973 your result will be as correct as possible, the only remaining reason for lack of accuracy being fact that you have no idea what isotopes constitute remaining 0.01% of the lead.

--
 
  • #25
Yea that makes sense. How did you get the 203.9... I got it being something around 207.
 
  • #26
According to wolfram page you linked to earlier, 203.9... is a correct atomic mass of ^{122}_{82}Pb.
 
  • #27
Ok so here is what I have right now:

82p, 122n --> 204 mass number (.0137) %
82p, 124n --> 206 mass number (.2625) %
82p, 125n --> 207 mass number (.2082) %
82p, 126n --> 208 mass number (.5155) %

(204*.0137) + (206*.2625) + (207*.2082) + (208*.5155) = approximate atomic mass of lead
(2.795) + (54.08) + (43.10) + (107.2) = approximate atomic mass of lead
(a) 207.2 amu = approximate atomic mass of lead

This is what the directions say (a) Using these data, calculate the approximate atomic mass of lead; (b) Why is this number in (a) only approximate?

I'm still not sure why the number in (a) is only approximate of the atomic mass of lead. Is it because like someone said before, that we don't know what the .01% of the isotope is?
I'm really not sure
 
  • #28
Mass number and atomic mass of the isotope are DIFFERENT. You have calculated average using MASS NUMBERS which are incorrect, so your result must be incorrect.
 
  • #29
Oh. How do I do it using atomic mass?
 
  • #30
Exactly the same way, but using atomic mass instead of mass number.
 

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