Asked by Anon

On another planet, the isotopes of titanium have the following natural abundances.
Isotope 46Ti Abundance 70.900% Mass(amu) 45.95263

Isotope 48Ti Abundance 10.000% Mass(amu) 47.94795

Isotope 50Ti Abundance 19.100% Mass(amu) 49.94479

What is the average atomic mass of titanium on that planet?

I got 46.9 amu but it is wrong.
Answered by DrBob222
(45.95263*0.7090) + (47.94795*0.10) + (49.9479*0.191) = ?
Answered by Anonymous
15.64
Answered by Anonymous
i have no idea
Answered by PooFace
You forgot your significant figures.
Answered by V
46.70 amu
Answered by Anonymous Chem Major Student (:
.70900 x 45.95263 = 32.580
.10000 x 49.94479 = 4.7948
.19100 x 49.94479 = 9.5395
*(Be aware that these answers must have 5 significant figures)

32.580 + 4.7948 + 9.5395 = 46.918
*(Be aware that the final answer must go to 3 decimal places)
Answered by Bukola
46.83
Remember that while calculating you are not suppose to approximate not until you arrive at your final answer.
Answered by Bukola
I'm sorry I posted the right answer to the wrong question
Answered by Me
46.713 you welcomw
Answered by Alex
It’s 46.811 u
Answered by frank
46.627 u is the correct answer

There are three isotopes of titanium present, 46Ti, 48Ti, and 50Ti, so there are three terms in the weighted average equation.

average atomic mass=(45.95263 u×74.500%100%)+(47.94795 u×17.200%100%)

+(49.94479 u×8.300%100%)

average atomic mass=46.627 u
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