Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 2 - Atoms, Molecules, and Ions - Exercises - Page 74: 2.12a


6.116 grams of sulfur

Work Step by Step

You start with 6.500 g of hydrogen sulfide (chemical formula: H$_{2}$S) and if since it decomposes into only 2 elements, the amount of one element can be determined by subtracting the amount of the other element from the total mass. If 0.384 g of hydrogen is produced, 6.500 g - 0.384 g = 6.116 g of sulfur produced.
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