Calculate the atomic weight of element carbon (C), and element uranium (U). The isotope abundance: 12C,...
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.
Homework Answers
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Calculate the atomic weight of element carbon (C), and element
uranium (U).
The isotope abundance: 12C,...
Q37. Carbon has 2 stable isotopes 12C and 13C. The relative abundance of those isotopes is...
Q37. Carbon has 2 stable isotopes 12C and 13C. The relative abundance of those isotopes is 98.9% and 1.1% respectively. Determine the average mass of Carbon. Q38. An unknown element Q has two known isotopes: 60Q and 63Q. If the average atomic mass is 61.5 amu, what are the relative percentages of the isotopes?
Enter your answer in the provided box. The 235U isotope (atomic mass = 235.00) undergoes fission when bombarded with ne...
Enter your answer in the provided box. The 235U isotope (atomic mass = 235.00) undergoes fission when bombarded with neutrons. However, its natural abundance is only 0.72 percent. To separate it from the more abundant 238U isotope (atomic mass = 238.00), uranium is first converted to UF, which is easily vaporized above room temperature. The mixture of 23SUF, and 238UF gases is then subjected to many stages of effusion. Calculate how much more quickly 235UF, effuses than 238UF. Give the...
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes...
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
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138...
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
The hypothetical element Q has an atomic weight of 124.8 AMU in the periodic table and...
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.
need some explaining plaz. ke ke 12. Calculate the atomic weight of Kelsium, a fictional element,...
need some explaining plaz.
ke ke 12. Calculate the atomic weight of Kelsium, a fictional element, if it consists of two isotopes with the following abundance and masses: 11.99 amu 66.00% 13.98 amu 34.0096 A. 11:44 amu B. 8.958 amu C. 13.01 amu D 12.67 amu E 25.97 amu 13. Which of the following can we conclude from the atomic weight of boron which is comprised of just boron-10 and boron-11? A Boron-11 is the most abundant isotope. B Boron-10...
QUESTION 3 Calculate the average atomic mass of silver using the following da Isotope Abundance Mass...
QUESTION 3 Calculate the average atomic mass of silver using the following da Isotope Abundance Mass 107 Ag 51.84% 106.9051amu 109 Ag 48.16% 108.9048amu 106.91 amu 107.87 amu O 108.00 amu 107.90 amu 108.90 amu
Calculate the average atomic mass of lithium using the following data: Isotope Abundance Mass Li 7.5%...
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
Calculate the atomic mass of Carbon: 11. Calculate the atomic mass of Carbon 12C 14, 1"C...
Calculate the atomic mass of Carbon:
11. Calculate the atomic mass of Carbon 12C 14, 1"C 13 12.00000 98.89% 13.00335 1.11% 14.0 t-5715yrs
. (_92^235)U is a fissile isotope of uranium, used in the atomic bomb dropped on Hiroshima...
. (_92^235)U is a fissile isotope of uranium, used in the atomic bomb dropped on Hiroshima in 1945. The critical mass is 56 kg. The primary isotope is not fissile and had to be removed by a process which required synthesis of UF6, a gas. How much 235UF6 was required to produce a critical mass of the element? [Molar masses: U, 235.0439 g; F, 18.9984 g]
Enter your answer in the provided box. The 235U isotope (atomic mass = 235.00) undergoes fission when bombarded with neutrons. However, its natural abundance is only 0.72 percent. To separate it from the more abundant 238U isotope (atomic mass = 238.00), uranium is first converted to UF, which is easily vaporized above room temperature. The mixture of 23SUF, and 238UF gases is then subjected to many stages of effusion. Calculate how much more quickly 235UF, effuses than 238UF. Give the...
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
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
need some explaining plaz.
ke ke 12. Calculate the atomic weight of Kelsium, a fictional element, if it consists of two isotopes with the following abundance and masses: 11.99 amu 66.00% 13.98 amu 34.0096 A. 11:44 amu B. 8.958 amu C. 13.01 amu D 12.67 amu E 25.97 amu 13. Which of the following can we conclude from the atomic weight of boron which is comprised of just boron-10 and boron-11? A Boron-11 is the most abundant isotope. B Boron-10...
QUESTION 3 Calculate the average atomic mass of silver using the following da Isotope Abundance Mass 107 Ag 51.84% 106.9051amu 109 Ag 48.16% 108.9048amu 106.91 amu 107.87 amu O 108.00 amu 107.90 amu 108.90 amu
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
Calculate the atomic mass of Carbon:
11. Calculate the atomic mass of Carbon 12C 14, 1"C 13 12.00000 98.89% 13.00335 1.11% 14.0 t-5715yrs
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