8) A pure sample of an element was vaporized and injected into a mass spectrometer and the data was plotted on the graph below. The mass values for the isotopes were found to be: A-24 (23.985 amu), A-25 (24.986 amu), and A-26 (25.983). Find the average atomic mass and identify the element. 78.99 Percent Abundance 90 SO 70 60 50 40 30 20 10 0- gr 24 10.00 11.01 26 25 Mass Number 0.00 27 Show proper work!

A hypothetical element, M, with average atomic weight of 35.75. M has three stable isotopes with the masses and percentage abundances are shown below. Identify missing information on the table. Isotopes Mass (amu) Abundance 34M 33.99 46.78 37M ? 33.93 38M 37.96 ? 3/M mass = 36.87 amu, 38M percentage abundance = 19.64%. 37 'M mass = 36.29 amu, 38M percentage abundance = 19.89%. %3D 3/M mass = 36.92 amu, 38M percentage abundance = 19.29%. 37M mass = 36.92 amu, 38M percentage abundance = 20.29%. %3D %3D 37 'M mass = 32.92 amu, 3ºM percentage abundance = 19.29%.

The element zirconium has five naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. Show your work to determine the average atomic mass. Isotope           Mass %           Abundance Zr-90              89.9043             51.40 Zr-91             90.9053              11.20 Zr-92             91.9046               17.10 Zr-94             93.9061              17.50 Zr-96            95.9082                   2.80

An element has three naturally occurring isotopes with the following masses and abundances: Isotopic Fractional Mass Abundance (ати) 19.992 0.9048 20.994 0.0027 21.991 0.0925 Calculate the atomic weight of this element. What is the identity of the element? Atomic weight amu Element is

Using the following data, determine the percent abundance of the third isotope and the average atomic mass of isotope X. Give as a percentage. X-22 atomic mass = 22.10498 abundance = 52.3985% X-23 atomic mass = 23.0005 abundance = 24.8731% X-24 Atomic mass = 24.0593

Element A has two isotopes. The first isotope is present 19.41% of the time and has a mass of 231.12. The second isotope has a mass of 193.24. Calculate the atomic mass of element A.

Naturally occurring neon exists as three isotopes. 90.51% is Ne-20 with a mass of 19.99 amu, O.27% is Ne-21 with a mass of 20.99 amu, and9.22% is Ne-22 with a mass of 21.99 amu. What is the atomic mass of neon? O 20.18 amu O 62.97 amu O 10.00 amu O 20.99 amu

A hypothetical element exists as two isotopes: I = 68.00 amu and II = 71.00 amu. If the percent abundance of isotope I is (6.61x10^1)%, what would be the calculated atomic mass (in amu)?

A certain element has five stable isotopes with the following masses and percent abundance: Isotope 1:   63.929147 amu,   48.63% Isotope 2:   65.926037 amu,   27.90% Isotope 3:   66.927131 amu,    4.100% Isotope 4:   67.924848 amu,   18.75% Isotope 5:   69.925325 amu,     0.6200%      What is the atomic mass of this element? (Do not round intermediate calculations.)

6) Complete the following table by calculating the atomic mass. Isotope Mass of Atom (u) Percent Abundance (%) ¹H 2H 12C 13C 160 170 180 1.007825 2.1040 12.0 13.003355 15.994915 16.999131 17.999160 99.985 0.015 98.90 1.10 99.762 0.038 0.200 Atomic Mass (u)