Chromium has an atomic mass of 51.9961 u and consists of four isotopes, 50 Cr, 52Cr,...
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 element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
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 Relative abundance (amu) (%) 78.9 82.9 13.0 120 869 750 Express your answer to three significant figures and include the appropriate units.
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 77.100% 45.95263 48Ti 16.500% 47.94795 50Ti 6.400% 49.94479 46Ti What is the average atomic mass of titanium on that planet? average atomic mass = JE TOOLS xio
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (u) 46Ti 73.800% 45.95263 48Ti 18.900% 47.94795 50Ti 7.300% 49.94479 What is the average atomic mass of titanium on that planet? average atomic mass = also round to the correct amount of Significant Figures
8 of 50 > Suppose a new element with an average atomic mass of 23.873 u is discovered on Mars. This element is composed of two isotopes. The most abundant isotope has a natural abundance of 83.664% and an isotopic mass of 22.821 u. Calculate the isotopic mass of the least abundant isotope. isotopic mass:
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
Antimony has two naturally occuring isotopes, 121Sb and 123Sb. 121Sb has an atomic mass of 120.9038 u, and 129Sb has an atomic mass of 122.9042 u. Antimony has an average atomic mass of 121.7601 u. What is the percent natural abundance of cach isotope? 121 Sb: 1235b:
Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a...