10- What is the atomic mass of lithium, if it has two naturally occurring isotopes, gli...
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
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%
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 =
5) Calculate the atomic mass of an imaginary element X that has 3 naturally occurring isotopes with the following masses and natural abundances: 106.90509 amu 108.90476 amu 107.91536 amu 51.84% 38.46% 9.70% A) 106.80 amu B) 108 amu C) 107.77 amu D) 108.32 amu E) 107.8 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
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 Oxygen consists of three naturally occurring isotopes with masses 15.949915, 16.999131, and 17.999159 amu. The relative abundances of these three isotopes are 99.76, 0.03800, and 0.2000 percent, respectively. From these data calculate the average atomic mass of Oxygen (in amu).
Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a...