Log in
Chemistry
1
answer
0
watching
662
views

Copper metal dissolves in a silver nitrate solution. The balanced equation for the reaction is:

Cu(s) + 2AgNO3(aq) -------> Cu(NO3)2(aq) + 2Ag(s)

A. Starting with 150.ml of 0.250M silver nitrate, AgNO3, how many moles of AgNO3 is that?

B. If a 1.00g of copper metal is added to the solution would it all dissolve? Justify your answer.

Watch
1
answer
0
watching
662
views

For unlimited access to Homework Help, a Homework+ subscription is required.

John Edward Cayas
John Edward CayasLv10
6 Nov 2020

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Copper metal dissolves in a silver nitrate solution. The balanced equation for the reaction is:

A. Starting with 150.0 mL of 0.250 M silver nitrate, AgNO3, how many moles of AgNO3 is that?

B. If a 1.00 g of copper metal is added to the solution, would it all dissolve? Justify your answer.

Copper forms two different cations, cuprous (Cu+) and cupric (Cu2+). When solid copper reacts with silver nitrate solution, two reactions are possible, as shown in equations a and b.a) Molecular Equation: Cu(s) + AgNO3(aq) ? CuNO3(aq) + Ag(s)Net Ionic Equation: Cu(s) + Ag+(aq) ? Cu+(aq) + Ag(s)b) Molecular Equation: Cu(s) + 2AgNO3(aq) ? Cu(NO3)2(aq) + 2Ag(s)Net Ionic Equation: Cu(s) + 2Ag+(aq) ? Cu2+(aq) + 2Ag(s)1. What mass of metallic silver can form from 1.347 g of copper metal according to Equation a?2. What mass of metallic silver can form from 1.347 g of copper metal according to Equation b?3. A student reacts 1.347 g of copper with a solution containing excess silver nitrate andrecovers 2.248 g of silver metal. Which reaction, a) or b), most likely occurred in theexperiment? Explain your answer completely.

Copper metal dissolves in a silver nitrate solution. The balanced equation for the reaction is:

   

A. Starting with  of silver nitrate, , how many moles of is that?

B. If a of copper metal is added to the solution would it all dissolve? Justify your answer. (hint: what does a balanced equation allow you to do?)

copper wire and silver nitrate balanced equation

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in