Please quickly QUESTION 8(a) In the certain hydrated salt MS03-4H20, the mass percentage of H20 is 44.71%.Identify the element M in the salt?(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 was found to be 30.27%.The complete combustion of 1.367 g this compound produces 1.765 g of sulfur dioxide(SO2)() Determine the empirical formula for this compound.(H) If a sample of this compound having the mass 3.781 x 10 mg contains 9.528 x 10 molesof the compound, determine the molecular formula.

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(a) In the certain hydrated salt MSO3-4H20, the mass percentage of H20 is 44.71%. Identify the element M in the salt?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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QUESTION 8
(a) In the certain hydrated salt MS03-4H20, the mass percentage of H20 is 44.71%.
Identify the element M in the salt?
(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 was found to be 30.27%.
The complete combustion of 1.367 g this compound produces 1.765 g of sulfur dioxide
(SO2)
() Determine the empirical formula for this compound.
(H) If a sample of this compound having the mass 3.781 x 10 mg contains 9.528 x 10 moles
of the compound, determine the molecular formula.

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