Chlorine is found as two isotopes, Cl-35 and Cl-37 (or and Cl). The atomic mass of the Cl-35-isotope is 34,96885 amu while the Cl-37-isotope has an atomic mass equal to 36,96590 amu ( The textbook use this unit for atomic mass, we could as well have used the recommended unit «u»). In the Periodic Table given in the textbook the molar mass of Chlorine is given as 35,45 g/mol.
What is the percentage abundance of the two chlorine isotopes?
Chlorine is found as two isotopes, Cl-35 and Cl-37 (or and Cl). The atomic mass of...
There are two naturally occurring isotopes of chlorine. 35^CI has a mass of 34.9689 amu. 37^CI has a mass of 36.9659 amu. Determine the abundance of each isotope.
Question 3 (2.5 points) Chlorine has two naturally occurring isotopes. The isotope C1-35 (mass = 35.0 amu) makes up 75.8% of the sample, and the isotope CH-37 (mass = 37.0 amu) makes up 24.2% of the sample. What is the average atomic mass for chlorine? A) 36.0 amu B) 35 amu C) 36.6 amu D) 35.5 amu E) 35.521 amu
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.
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...
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.
The atomic mass of magnesium on the periodic table is based on three isotopes, ^24_12Mg, ^25_12Mg, and^26_12Mg. If a fourth isotope is discovered, it would change the abundances of all the others, and it would change the molar mass listed on the periodic table. Calculate the molar mass of magnesium, based on the masses and abundances given below.[^23_12Mg mass = 22.9862, abundance 22.50%] [^24_12Mg mass = 23.9850, abundance 62.49%] [^25_12Mg mass = 24.9858, abundance 10.20%]^26_12Mg mass = 25.9826, abundance 4.810%]
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 %
Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a...
Chlorine has two stable isotopes, 35Cl and 37Cl. If a sample of chlorine has an average molar mass of 36.19 g/mol, what percent of the sample is composed of the lighter isotope, 35Cl? The exact masses of the isotopes can be found at http://en.wikipedia.org/wiki/Isotopes_of_chlorine
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.