5) Calculate the atomic mass of an imaginary element X that has 3 naturally occurring isotopes...
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%
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
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.
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 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 =
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is _ _amu. Isotope Abundance (%) Mass (amu) 221X 74.22 220.90 12.78 220.00 2187 13.00 218.10 2207 219.70 220.34 220.43 219.00 33.333
Enter your answer in the provided box. An element has two naturally occurring isotopes. The mass numbers of these isotopes are 109 amu and 111 amu, with natural abundances of 35% and 65%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place. amu
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes are shown in the table below. Isotope 12c isotopic mass (amu) Abundance (%) 12.00 13.00 98.93 1.07 Calculate the average atomic mass of carbon to two digits after the decimal point. Number = _______ amu
2. An element has 2 naturally occurring isotopes with the following masses and abundances A. Calculate the atomic weight of the element. (20 pts) Isotope mass Percentage 34.97 amu 75.78% 36.97 amu 24.22% B. What is the element? C. How many neutrons does the heavier isotope have? (Round to whole number) D. How many electrons does the element have? E. What type(metal/nonmetal) of element is it? F. If the element above gains 1 electron what neutral element has the some...
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)