Chemistry: The Central Science (13th Edition)

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

Chapter 4 - Reactions in Aqueous Solution - Exercises: 4.51b

Answer

Al is oxidized Fe is reduced

Work Step by Step

3Fe(NO3)2 + 2Al --> 3Fe + 2Al(NO3)3 Al and Fe are in their elemental states so they are both oxidation state of 0. NO3-, the nitrate ion has a charge of -1 so on the left since there are 2 (NO3)- groups, which equals -2 then Fe must be Fe2+ Therefore, Fe goes from 2+ on the left to 0 on the right Fe gains electrons and is reduced Al(NO3)3. Here we have 3 (NO3)- groups, which is 3- so that means Al is Al3+ Therefore, Al goes from 0 to 3+ Al loses electrons and is oxidized
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