Textbook Question
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (b) What is the net ionic equation that describes this reaction?
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6. Chemical Quantities & Aqueous Reactions
Activity Series
Multiple Choice
Based on the activity series, which of the following metals will displace copper from a solution of copper(II) sulfate?
A
Mercury
B
Gold
C
Silver
D
Zinc
Verified step by step guidance1
Understand that the activity series is a list of metals ranked by their ability to lose electrons (oxidize) and displace other metals from their compounds in solution.
Recall that a metal can displace another metal from its compound if it is higher in the activity series, meaning it is more reactive and more easily oxidized.
Identify the position of copper in the activity series and compare it with the metals given: mercury, gold, silver, and zinc.
Note that zinc is above copper in the activity series, indicating that zinc can lose electrons more readily and thus displace copper from copper(II) sulfate solution.
Conclude that mercury, gold, and silver are below copper in the activity series and therefore cannot displace copper from its solution.
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