QUESTION 3 Calculate the average atomic mass of silver using the following da Isotope Abundance Mass...
Calculate the average atomic mass of silver using the following data: Isotope Abundance Mass 51.84% 106.9051amu 109 Ag 48.16% 108.9048amu 107 Ag
Calculate the average atomic mass of lithium using the following data: Isotope Abundance Mass Li 7.5% 16.0151 amu Li 92.5% 7.0160 aum
Silver has two naturally occuring isotopes, and its average atomic mass is 107.87 u. The natural abundance of 107Ag is 51.84%. What is the other naturally occuring isotope of silver?(a)105Ag (b)106Ag (c)108Ag (d)109Ag
Silver has two naturally occurring isotopes: Ag−107Ag−107 with a mass of 106.905 amu and a natural abundance of 51.84 %%, and Ag−109Ag−109. Use the atomic mass of silver listed in the periodic table to determine the mass of Ag−109Ag−109. Express your answer to four significant figures and include the appropriate units.
Given the following isotopes for oxygen and their percent abundance calculate oxygen's average atomic mass. (Show Work) Isotope Abundance 160 99.76% 120 0.04% 0.2% 180
33. (5 points) Calculate the average atomic mass of strontium, Sr, from the data below. Isotope Sr Mass (amu) 83.9134 Natural Abundance (%) 0.5601 Sr 85.9093 9.862 86.9089 7.000 Sr 87.9056 82.578 09
Calculate the atomic weight of element carbon (C), and element uranium (U). The isotope abundance: 12C, 98.90%; 13C (13.00335 amu), 1.10%; 238U (238.05078 amu), 99.28%; 235U (235.04392 amu), 0.72%, assuming 14C and 234U are negligible.
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (amu) 46Ti 77.100% 45.95263 48Ti 11.700% 47.94795 50Ti 11.200% 49.94479 What is the average atomic mass of titanium on that planet? _______=amu
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
Review Constants Periodic Table Part A Atomic mass is a weighted average of the masses of the naturally occurring isotopes of that element. For example, consider isotopes of lithium: Abundance Mass Isotope (%) (amu) Li 7.5 6.015 On a mission to a newly discovered planet, an astronaut finds copper abundances of 69.15 % for Cu and 30.85 % for 65Cu. What is the atomic mass of copper for this location? The mass of Cu is 62.9300 amu . The mass...