Calculate the mass that would be listed for an element which contains 4 atoms of atomic...
Part A What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%) 1 81.9 12.2 2 84.9 15.0 3 88.9 72.8 Express your answer to three significant figures and include the appropriate units. Part B What is the relative atomic mass of the element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%)...
The atomic mass of ^63Cu is 62.9296 amu and the atomic mass of ^65Cu is 64.9278 amu. In a natural sample, 69.10% of the atoms are ^63Cu, and 30.90% are ^65Cu. Calculate a value for the molar mass of copper in g mol-1, given one atomic mass unit (amu or u) equals 1.66054x10^-24g.
Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following masses and natural abundances. X-45, 44.8776 amu, 32.88% X-47, 46.9443 amu, 67.12%
5) Calculate the atomic mass of an imaginary element X that has 3 naturally occurring isotopes with the following masses and natural abundances: 106.90509 amu 108.90476 amu 107.91536 amu 51.84% 38.46% 9.70% A) 106.80 amu B) 108 amu C) 107.77 amu D) 108.32 amu E) 107.8 amu
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689 amu and a percent natural abundance of 75.53 %. The second has an atomic mass of 36.9474 amu and a percent natural abundance of 24.47 %. What is the atomic weight of the element? amu
An element has three naturally occurring isotopes with masses as listed below. The average atomic mass of this element is 28.08 amu. Determine the two missing percent abundances.^28X 27.98 amu % abundance =^29X 28.98 amu % abundance = 4.68 %^30X 29.97 amu % abundance =
Question 4 2 pts What is the average atomic mass of the element that has the following isotopes? 0.005% is of mass 234.040947 amu 0.720% is of mass 235.043924 amu 99.275% is of mass 238.050784 amu Once you find the average atomic mass, please find which element on the periodic table has that mass. Type the atomic symbol (one or two letters only, starting with a capital letter) here. Thank you.
4. An element has two naturally occurring isotopes. The mass numbers of these isotopes are 111 amu and 113 amu, with natural abundances of 25% and 75%, respectively. Calculate the atomic mass for this element. 6 pts
Saturdy occurring Stan imaginary element) consists of 24.13% St-100 atoms (mass 100.90 amu), 12.22% SF-102 atoms (mass 102.90 amu), 28.73% Sf.103 atoms (mass (103.90 amul and 7.49% Sf-105 atoms (mass 100.90 Calculate the average atomic mass of Sf. Show your work to receive credit.
Element X has two natural isotopes: X-6 (6.015 amu) and X-7 (7.016 amu). Calculate the atomic mass of element X given the abundance of X-7 is 92.5%. a. 6.09 amu b. 6.50 amu 6.52 amu d 6.94 amu e. 12.5 amu