What are possible relative percentages abundance’s of two isotopes of lanthanum? One isotope has an atomic mass of 137.9071u (Lanthanum-138) and the other has an atomic mass of 138.9083u (Lanthanum-139).
What are possible relative percentages abundance’s of two isotopes of lanthanum? One isotope has an atomic...
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...
rest from Consider the 2000 kg car shown below. The car coasts, from rest a height of 35 m. Determine (a) how fast the car is going when reaches the flat road below. When it reaches point A, the driver locks up the brakes. If the car comes to rest at point B, determine the coefficien lof static friction between the tires and the road as the car iskids to a stop. Determine the work done by the frictional force....
Chlorine has two isotopes. The lighter one has an atomic mass of 34.969 atomic mass units (amu), and the heavier has a mass of 36.966 amu. If the average atomic mass on another planet is 35.625 amu, what percentage is the lighter isotope? Give your answer to the nearest whole percent.
1. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu, and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042, and a relative abundance of 42.6%. Find the atomic mass of this element and identify it by name and symbol.
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.
8. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042 amu. Find the atomic mass of this element and, by comparison to the periodic table, identify it.
Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and a relative abundance of 69.17%. Use the atomic mass of copper to determine the mass of the other copper isotope. Express your answer using four significant figures.
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?
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
The table below shows the atomic masses of the two naturally occurring isotopes of rubidium. Isotope Atomic Mass (amu) 85Rb 84.912 87Rb 86.909 The average atomic mass of rubidium is 85.468 amu. What is the percent abundance of each isotope? 85Rb % 87Rb %