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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.

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Greg Montoya
Greg MontoyaLv10
8 Dec 2020

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Related questions

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

When 1.00 g of copper metal was placed in 50.0mL of .800M silver nitrate solution, 3.21g of silver metal were collected. The unbalanced equation for this reaction is: Cu(s) + AgNO3 (aq) ------> Cu(NO3)2 (aq) + Ag (s)

1. How many moles of copper were present?

2. How many moles of silver were produced?

3. What is the simplest whole number mole ratio between copper and silver?

4. What are the stoichiometric coefficients for each of the reactants and products?

5. How many moles of silver nitrate were initally present?

6. Based on the number of moles of copper and silver nitrate initially present, which one is the limiting reactant?

A 25g piece of copper (Cu) metal is placed in an aqueous silver nitrate (AgNO3) solution. The copper dissolves to form Cu2+ ions and the silver Ag+ ions plate out as solid silver on the piece of copper. After a short period of time, the weight of the piece of copper with silver deposit is 28.2 g. How many grams of silver are depostied on the piece of copper?

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