A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689...
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...
Use the References to access important values if needed for this question A certain element consists of two stable isotopes. The first has a mass of 68.9 amu and a percent natural abundance of 60.4 %. The second has a mass of 70.9 amu and a percent natural abundance of 39.6%. What is the atomic weight of the element a mu Submit Answer Retry Entire Group 9 more group attempts remaining
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
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
Part A What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%) 1 81.9 12.2 2 84.9 15.0 3 88.9 72.8 Express your answer to three significant figures and include the appropriate units. Part B What is the relative atomic mass of the element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%)...
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 nitrogen has two naturally occuring isotopes. One of these has a mass of 14.003 amu and a natural abundance of 99.63%; the other isotope has a mass of 15.00 and a natural abundance of 0.37%. Calculate the atomic mass of nitrogen.
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
S A certain element exists as three natural isotopes as shown in the table below. Isotope Mass (amu) Percent natural abundance 19.99244 90.51 20.99395 0.27 21.99138 9.22 Mass number 20 21 22 Calculate the average atomic mass of this element.
Part A What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass Relative abundance (amu) (%) 78.9 82.9 13.0 120 869 750 Express your answer to three significant figures and include the appropriate units.