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Suppose a new element is discovered and it has two stable isotopes. One isotope has a mass of 71.139 u and an abundance of 37.15% . The average atomic mass of the element is 74.353 u . What is the mass of the second isotope?
Suppose a new element is discovered and it has two stable isotopes. One isotope has a mass of 72.550 u and an abundance of 38.44%. The average atomic mass of the element is 70.565 u. What is the mass of the second isotope? mass of isotope: about us creen privacy policy terms of use contact us help
A new element, X, was recently discovered with the following isotopes: isotopes %natural abundance Mass (amu) X-107 8.971 106.8067 X-109 71.022 109.9231 X-110 20.007 110.2118 What is the atomic mass of X that should be reported on the periodic table?
A hypothetical element consists of two slopes. The abundance of one isotopes 76.00% and is atomic mass is 70.9802 Theomic mass of the second scope is 78.0782 What is the average atomic mass of the element? A 89.7190 3.76.3747 C. 74.5252 0.140.050 E72.6037
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
Element A has two isotopes. The first isotope is present 36.76% of the time and has a mass of 139.31. The second isotope has a mass of 111.16. Calculate the atomic mass of element A. (To two decimals places)
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
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.
8 of 50 > Suppose a new element with an average atomic mass of 23.873 u is discovered on Mars. This element is composed of two isotopes. The most abundant isotope has a natural abundance of 83.664% and an isotopic mass of 22.821 u. Calculate the isotopic mass of the least abundant isotope. isotopic mass:
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.
the element X has naturally occurring isotope. The masses (amu) and % abundance of the isotopes are given below. the average atomic mass of the element is ? Isotope: 221X, 220X, 218 X Abundance: 74.22, 12.78, 13.00 Mass: 220.9, 220.0, 218.1