(b) A certain element has two naturally occurring isotopes.The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%.The mass of the second isotope is 108.883 amu.Calculate the average atomic massWrite the chemical symbols of the isotopes(c) An organic compound consists of carbon, hydrogen and sulfur only.The percentage of carbon by mass in this compound wąs found to be 30.27%.The complete combustion of 1.367 g this compound produces 1.765 g of sulfur dioxide(SO2)(i) Determine the empirical formula for this compound.(ii) If a sample of this compound having the mass 3.781 x 103 mg contains 9.528 x 10-3 molesof the compound, determine the molecular formula.

Chemical symbol of isotopes are :- 107Ag and 109Ag.

(b) A certain element has two naturally occurring isotopes. The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%. The mass of the second isotope is 108.883 amu. Calculate the average atomic mass Write the chemical symbols of the isotopes

(b) A certain element has two naturally occurring isotopes. The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%. The mass of the second isotope is 108.883 amu. Calculate the average atomic mass Write the chemical symbols of the isotopes

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

Section: Chapter Questions

Problem 2.CCP

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(b) A certain element has two naturally occurring isotopes.
The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%.
The mass of the second isotope is 108.883 amu.
Calculate the average atomic mass
Write the chemical symbols of the isotopes
(c) An organic compound consists of carbon, hydrogen and sulfur only.
The percentage of carbon by mass in this compound wąs found to be 30.27%.
The complete combustion of 1.367 g this compound produces 1.765 g of sulfur dioxide
(SO2)
(i) Determine the empirical formula for this compound.
(ii) If a sample of this compound having the mass 3.781 x 103 mg contains 9.528 x 10-3 moles
of the compound, determine the molecular formula.

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