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Question 4 2 pts What is the average atomic mass of the element that has the...
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.
8. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042 amu. Find the atomic mass of this element and, by comparison to the periodic table, identify it.
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 =
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
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
Suppose you are trying to construct a periodic table in an alternate universe. You discover element "X", which has two isotopes. Isotope #1 has a mass of 14.02 amu and an abundance of 29.5%. Isotope #2 has a mass of 15.02 amu. What atomic mass would you put on the periodic table for element "X"? Please show all working out and neat hand writing please. Thank you.
The average atomic mass of a hypothetical element is 139.85 amu. Determine the missing abundances of isotopes using the information provided. % Abundance 2.40 Isotope 1 2 3 WN Mass (amu) 135.8653 137.9946 139.9071 141.9023 3.50 ? ? 4
An unknown element (Element X) has three naturally occurring isotopes. Complete the table by filling in the missing percent abundance (2 decimal places). Then calculate the atomic mass of element X (1 decimal place) and determine its identity by filling in its atomic symbol (case sensitive). Isotope Abundance (%) Atomic Mass (amu) 23.985042 1 78.99 2 24.985837 10.00 3 25.982593 amu Atomic mass of element X (1 decimal place): Atomic symbol of element X:
1. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu, and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042, and a relative abundance of 42.6%. Find the atomic mass of this element and identify it by name and symbol.
< Question 4 of 17 > Suppose that a fictitious element, X, has two isotopes: 59X (59.015 amu) and "x (62.011 amu). The lighter isotope has an abundance of 75.7%. Calculate the average atomic mass of the element X average atomic mass: