The atomic weight is the weighted average of the abundance of isotopes in nature.
so for lanthanum the mass of lanthanum 139 has the mass as given below
(138 X .089%) + ( 139 X 99.9%) = 138.906 amu
for second materials which has two isotopes 113 and 115 e atomic weight of the element is
= (113 X 4.28 %) + ( 115 X 95.7 %) = 114.89 amu
The last question is the repeat of second question
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138...
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
rest from Consider the 2000 kg car shown below. The car coasts, from rest a height of 35 m. Determine (a) how fast the car is going when reaches the flat road below. When it reaches point A, the driver locks up the brakes. If the car comes to rest at point B, determine the coefficien lof static friction between the tires and the road as the car iskids to a stop. Determine the work done by the frictional force....
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.
What are possible relative percentages abundance’s of two isotopes of lanthanum? One isotope has an atomic mass of 137.9071u (Lanthanum-138) and the other has an atomic mass of 138.9083u (Lanthanum-139).
Use the References to access important values if needed for this question A certain element consists of two stable isotopes. The first has a mass of 68.9 amu and a percent natural abundance of 60.4 %. The second has a mass of 70.9 amu and a percent natural abundance of 39.6%. What is the atomic weight of the element a mu Submit Answer Retry Entire Group 9 more group attempts remaining
The hypothetical element Q has an atomic weight of 124.8 AMU in the periodic table and only has two stable isotopes. Q isotope 1 has an abundance of 55.83 % and an isotopic mass of 122.16 AMU. What is the mass of Q isotope in AMU ? Round 3 decimal places.
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 nitrogen has two naturally occuring isotopes. One of these has a mass of 14.003 amu and a natural abundance of 99.63%; the other isotope has a mass of 15.00 and a natural abundance of 0.37%. Calculate the atomic mass of nitrogen.
S A certain element exists as three natural isotopes as shown in the table below. Isotope Mass (amu) Percent natural abundance 19.99244 90.51 20.99395 0.27 21.99138 9.22 Mass number 20 21 22 Calculate the average atomic mass of this element.
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