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?
6. Chemical Quantities & Aqueous Reactions
Activity Series
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple 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.
1:11mWatch next
Master Single Displacement Reactions with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Activity Series practice set
Problem sets built by lead tutorsExpert video explanations