Chemistry: A Molecular Approach (3rd Edition)

Published by Prentice Hall
ISBN 10: 0321809246
ISBN 13: 978-0-32180-924-7

Chapter 3 - Sections 3.1-3.12 - Exercises - Problems by Topic - Page 133: 85c



Work Step by Step

Convert the mass of each constituent element into moles by dividing by its molar mass: $1.443g\ Se\times\frac{1mol}{78.971g}=0.01827mol\ Se$ $5.841g\ Br\times\frac{1mol}{79.904g}=0.07310mol\ Br$ Formulas have whole number subscripts so divide all the amounts by the smallest and round if the number is really close. Then multiply by whatever factor makes them all a whole number or very close to a whole number. $\frac{0.01827mol\ Se}{0.01827}=1$ $\frac{0.0731mol\ Br}{0.01827}=4$ So the empirical formula for this compound is: $SeBr_{4}$
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