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?

Question

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?

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