Antimony, Sb, has two stable isotopes: 121Sb, 120.904u, and 123Sb, 122.904u. What is the percent abundance of 121Sb? (Tip: fractional abundances of isotopes must equal 1)
[1] 121.76
[2] 0.5720
[3] 57.20
[4] 0.4280
[5] I need more information to be able to answer this question
ANSWER:
Option (5) is the correct answer. We need more information to solve the question. If the percentage abundance of 123 Sb is given then the percentage abundance of 121 Sb can be calculated. Because the sum of the percentage of abundance is equal to 100. Similarly the percentage abundance of 121 Sb can be calculated if the fractional abundance of 123 Sb or 121 Sb is given. For example if the fractional abundance of 121 Sb is 0.5720 then the percent abundance is given as 0.5720 X 100 = 57.20 %
Similarly if fractional abundance of 123 Sb is given that of 121 Sb can be calculated. For example if the fractional abundance of 123 Sb is 0.4280. The fractional abundance of 121Sb is 1.000 - 0.4280 = 0.5720
Then the percentage abundance of 121Sb is given as = Fractional abundance X 100 = 0.5720 X 100 = 57.20 %
Antimony, Sb, has two stable isotopes: 121Sb, 120.904u, and 123Sb, 122.904u. What is the percent abundance...
Antimony has two naturally occuring isotopes, 121Sb and 123Sb. 121Sb has an atomic mass of 120.9038 u, and 129Sb has an atomic mass of 122.9042 u. Antimony has an average atomic mass of 121.7601 u. What is the percent natural abundance of cach isotope? 121 Sb: 1235b:
QUESTION 5 An element has 4 stable isotopes. The masses and percent abundances for the isotopes are m1 = 135.907 amu (0.185 %) m2 = 137.906 amu (0.251 %) m3 = 139.905 amu ( 88.450 %) m4 = 141.909 amu Based on this information, the chemical symbol for the element is , it has protons, and the number of neutrons in the heaviest isotope is
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
Silver has two stable isotopes with masses of 106.90509 a.m.u. and 108.9047 a.m.u. If the average atomic weight of silver was 108.2150 a.m.u. what would be the percent abundance of the LIGHTER isotope? Your percent abundance must be accurate to 0.01 to be receive credit.
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...
QUESTION 3 A fictitious element is composed of isotopes A and B with masses of 61.9887 and 64.9846 amu respectively. The average atomic mass of the element is 64.52 amu. What can you conclude about the natural abundances of the two isotopes? O The natural abundance of isotope A must be greater than that of isotope B OThe natural abundance of isotope B must be greater than that of isotope A. O The natural abundances of both isotopes must be...
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689 amu and a percent natural abundance of 75.53 %. The second has an atomic mass of 36.9474 amu and a percent natural abundance of 24.47 %. What is the atomic weight of the element? amu
Problem 42.40 Part A The element bromine has two stable isotopes: 79Br with an atomic mass of 78.92 u and 81 Br with an atomic mass of 80.92 u.A periodic table shows that the chemical atomic mass of bromine is 79.90 u What is the percent abundance of 79Br? Express your answer using two significant figures. The percent abundance of 79Br Submit Provide Feedback
Element X has two stable isotopes, 50X and 44X. One mole of X atoms weighs 48.57 grams. Identify the percent abundances of 50X and 44X. The answer is 24% for 44X and 76% for 50X. EXPLAIN IN DETAIL HOW YOU GOT THE ANSWER. Thank you.
1 (6)Uranium has three naturally occurring isotopes 22U, 235s2U, and 3 2U. The isotope Uranium-235is considered to be "weapons grade uranium" and can be used to make atomic weapons. The fractional abundances for two of the uranium isotopes are uranium-238-99.274% and Uranium-234-0.005%. The molecular mass of natural uranium is 237.9758amu. What is the fractional abundance of weapons grade uranium using these numbers (note: the number on the periodic table takes into account isotopes that aren't natural so use the numbers...