Potassium has three naturally occurring isotopes.  According to one source of data, Potassium-39 (mass 38.9637 amu) makes up 93.26%, potassium-40 (mass 39.9640 amu) makes up just 0.01%, and potassium-41 (mass 40.9618 amu) makes up 6.73%.  What is the average atomic mass of potassium based on these relative abundances?  Show all your work for credit, and express your final answer to 2 decimal places and include the unit.

An element has two naturally occurring isotopes. One has an abundance of 51.839% and an isotopic mass of 106.905093 AMU. The other has an abundance of 48.161% and an isotopic mass of 108.904756 AMU. What is the average atomic mass of the element?

An atom has a diameter of 2.50 Å and the nucleus of that atom has a diameter of 6.00 x 10-5 Å. Determine the fraction of the volume of the atom that is taken up by the nucleus. Assume the atom and the nucleus are a sphere. fraction of atomic volume: Calculate the density of a proton, given that the mass of a proton is 1.0073 amu and the diameter of a proton is 1.69 × 10-¹5 density: m. g/cm³

There are two naturally occurring isotopes of europium, 151Eu(151.0 amu) and 153Eu(153.0 amu). If the atomic mass of Eu is 151.96, what is the approximate natural abundance of 151Eu?

Part 1 As seen on the periodic table, the element silicon (Si) has an atomic mass of 28.086 amu. This element is composed of three naturally-occurring isotopes. The first isotope, silicon-28, has a mass of 27.977 amu and a natural abundance of 92.229%. The second isotope, silicon-30, has a mass of 29.974 amu and a natural abundance of 3.087%. What is the mass (in amu) of silicon's third isotope? write your final answer (with the correct significant figures) Part 2 Based on the answer for part 1, the name of the third isotope of silicon is ___. An atom of that particular isotope contains___ protons and ____ neutrons.

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

1- For each of the following atoms, calculate the number of protons and neutrons in the nucleus and the number of electrons outside the nucleus (assume neutral atoms). element number of number of number of electrons mass number (A) symbol 126C protons (Z) neutrons 12 10 12 10 14 27 10 23,1Na 11 17 18 2- Calculate the atomic mass to four significant figures for carbon, given the following data: Isotope Exact Atomic Mass (amu) 12.00000 13.00335 Abundance in Nature (%) 98.89 1.110 12C 13C

Calculated the weighted average of a substance from space. It has an abundance of 30.0% and 70.0% for its two isotopes. The atomic mass for the two isotopes are 111.653amu and 113.665amu, respectively.

Calculate the atomic mass of each of the isotopes listed below. Give your answer in grams (g). The values will include the mass of Z electrons. Use 1 u = 1.6605 X 10-24 g. 1) Calculate the atomic mass of the isotopes 1H in grams (g). The atomic mass m1H = 1.007825 u. (Express your answer to five significant figures.) 2) Calculate the atomic mass of the isotopes 4He in grams (g). The atomic mass m4He = 4.002602 u. (Express your answer to five significant figures.) 3) Calculate the atomic mass of the isotopes 12C in grams (g). The atomic mass m12C = 12.000000 u. (Express your answer to five significant figures.) 4) Calculate the atomic mass of the isotopes 56Fe in grams (g). The atomic mass m56Fe = 55.934940 u. (Express your answer to five significant figures.) 5) Calculate the atomic mass of the isotopes 238U in grams (g). The atomic mass m238U = 238.050784 u. (Express your answer to five significant figures.)

what is the atomic mass of an unidentified element that has 2 naturally occurring isotopes with the following masses and natural abundances?  Isotope 1: 44.8776 amu, 32.88%isotope 2: 46.9443 amu, 67.12%