Calculate the atomic weight for thallium. It has two naturally occurring isotopes, thallium-203 (202.972 u, 29.50% abundant) and thallium-205 (204.975 u, 70.50% abundant). and show your work.
Calculate the atomic weight for thallium. It has two naturally occurring isotopes, thallium-203 (202.972 u, 29.50%...
A hypothetical element X has 3 naturally occurring isotopes: 41.20% of 21X, with an atomic weight of 21.016 amu, 6.83% of 22X, with an atomic weight of 21.942 amu, and 51.97% of 24X, with an atomic weight of 23.974 amu. On the basis of these data, calculate the average atomic weight of element X. Report your answer to two decimal places.
4. The element boron has two naturally occurring isotopes. One has atomic mass 10.0129 u, while the other has atomic mass 11.0093 u. The average atomic mass of boron is 10.811 u. Determine the percentage occurrence of each isotope.
A fictitious element, Beaverium, has two naturally occurring isotopes. 285Bv has a mass of 284.67 amu and is 42.744% abundant. 288Bv has a mass of 287.73 amu and is 57.256% abundant. What is the average atomic mass (in amu) of Beaverium?
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%
has two naturally occurring isotopes, and, with masses of 78.9183 u and 80.9163 u, respectively. Calculate the percent abundances of these isotopes of bromine. Percent abundance of = % Percent abundance of = % Submit Answer Try Another Version 10 item attempts remaining Previous
An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 125 amu and 127 amu, with natural abundances of 80% and 20%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place. -------- amu
An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 111 amu and 113 amu, with natural abundances of 75% and 25%, respectively. Calculate its average atomic mass.
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
10- What is the atomic mass of lithium, if it has two naturally occurring isotopes, gli and li. Their masses and relative abundances are 6.0151 amu (7.49%) and 7.0160amu (92.51%) respectively. (5 points)
In another universe, element trinium has two naturally occurring isotopes, 34Tr and 35Tr. One of these has a natural abundance of about 10% and one is about 90%. If the atomic mass of trinium is 34.1 amu, what is most likely to be the isotope that is about 90% abundant? options: trinium-34 trinium-35