please help with the last one 11:43Done11 of 11Fe*2562624Cu*12934632927For the next two sections you must show all of your work forcredit.Average Atomic Mass Calculations1. The noble gas, neon, has three isotopes of masses, 22, 21, and 20.If the isotopes have the abundance 8.01%, 1.99% and 90.00%respectively, what is the average atomic mass of neon atoms?2. A naturally occurring same of an element consists of two isotopes,one of mass 85 and one of mass 87. The abundance of theseisotopes is 71% and 29%. Calculate the average atomic mass ofan atom of this element.3. If 6°Ga and 7"Ga occur in the %'s 62.1 and 37.9, calculate theaverage atomic mass of gallium atoms.Percent Abundance1. A sample of Germanium has an average mass of 72.63 amu. If thesample is composed of only Ge-70 and Ge-74, what is the percentabundance of each isotope?2. What is the relative abundance of each isotope present in a sampleof Tin if the average atomic mass of the sample is 118.711 amuand only contains isotopes Sn-118 and Sn-122?

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Answered: 2. What is the relative abundance of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section2.3: Isotopes And Average Atomic Mass

Problem 2.4CE

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An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.
Determine whether the statements given below are true or false. (a) The mass of an atom can have the unit mole. (b) In N204, the mass of the oxygen is twice that of the nitrogen. (c) One mole of chlorine atoms has a mass of 35.45 g. (d) Boron has an average atomic mass of 10.81 amu. It has two isotopes, B-10 (10.01 amu) and B-11 (11.01 amu). There is more naturally occurring B-10 than B-11. (e) The compound C6H12O2N has for its simplest formula C3H6ON1/2. (f) A 558.5-g sample of iron contains ten times as many atoms as 0.5200 g of chromium. (g) If 1.00 mol of ammonia is mixed with 1.00 mol of oxygen the following reaction occurs, 4NH3(g)+5O2(g)4NO(g)+6H2O(l)All the oxygen is consumed. (h) When balancing an equation, the total number of moles of reactant molecules must equal the total number of moles of product molecules.
The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
Chlorine has two isotopes, Cl-35 and Cl-37. Their abundances are 75.53% and 24.47%, respectively. Assume that the only hydrogen isotope present is H-1. (a) How many different HCI molecules are possible? (b) What is the sum of the mass numbers of the two atoms in each molecule? (c) Sketch the mass spectrum for HCI if all the positive ions are obtained by removing a single electron from an HCI molecule.
Neon is an inert gas with three stable isotopes. It is used in gas lasers and in advertising signs. Its isotopes and their abundances are: Ne-20 19.9924 amu 90.51% Ne-21 20.9938 amu 0.27% Ne-22 21.9914 amu 9.22% What is the average atomic mass of neon?
When a sample of phosphorus burns in air, the compound P4O10 forms. One experiment showed that 0.744 g of phosphorus formed 1.704 g of P4O10. Use this information to determine the ratio of the atomic weights of phosphorus and oxygen (mass P/mass O). If the atomic weight of oxygen is assumed to be 16.000, calculate the atomic weight of phosphorus.

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2. What is the relative abundance of each isotope present in a sample of Tin if the average atomic mass of the sample is 118.711 amu and only contains isotopes Sn-118 and Sn-122?