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Consider the reaction: Cu(s)+2 AgNO3(aq) = 2 Ag(s)+Cu(NO3)2(aq)


If 3.00 moles of copper metal react:


a) How many moles of silver metal will be produced?

b) How many grams of silver metal will be produced?

c) How many moles of copper (II) nitrate will be produced?

d) How many grams of copper (II) nitrate will be produced?

Respuesta :

Answer:

(a) 6 moles of Ag

(b) 647.22g of Ag

(c) 3 moles of copper (II) nitrate

(d)  564g of copper (II) nitrate

Explanation:

          Cu(s) + 2AgNO3(aq)= 2Ag(s) + Cu(NO3)2(aq)

(a)According to the above equation, 1 mole of Cu gives 2 mole of Ag. So, 3 moles of Cu will give:

Cu  :  Ag

 1       2

 3       x

x = 3*2

x = 6 moles of silver

(b) To find grams of silver metal, multiply the moles from (a) with its molar mass,

mass=no. of moles × MM

        = 6 × 107.87g

        = 647.22g of Ag will be produced

(c) According to the above equation, 1 mole of Cu gives 1 mole of Cu(NO3)2, so 3 moles of Cu will give:

Cu : Cu(NO3)2

 1         1

 3         x

x= 3 * 1

x = 3 moles of Cu(NO3)2

(d) To find grams of Cu(NO3)2, multiple moles with (a) with molar mass of Cu(NO3)2,

mass of Cu(NO3)2 = moles × MM

                              = 3 × 188g/mol

                              = 564g of Cu(NO3)2

CintiaSalazar

Taking into account the reaction stoichiometry:

  • 4 moles of silver metal will be produced.
  • 431.48 grams of silver metal will be produced.
  • 2 moles of copper (II) nitrate will be produced.
  • 375.08 grams of copper (II) nitrate will be produced.

Reaction stoichiometry

In first place, the balanced reaction is:

Cu + 2 AgNO₃  → 2 Ag + Cu(NO₃)₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • Cu: 1 mole
  • AgNO₃: 2 moles  
  • Ag: 2 moles
  • Cu(NO₃)₂: 1 mole

The molar mass of the compounds is:

  • Cu: 63.54 g/mole
  • AgNO₃: 169.87 g/mole
  • Ag: 107.87 g/mole
  • Cu(NO₃)₂: 187.54 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

  • Cu: 1 mole ×63.54 g/mole= 63.54 grams
  • AgNO₃: 2 moles ×169.87 g/mole= 339.74 grams
  • Ag: 2 moles 2 mole ×107.87 g/mole= 215.74 grams
  • Cu(NO₃)₂: 1 mole ×187.54 g/mole= 187.54 grams

Moles of silver produced

The following rule of three can be applied: If by reaction stoichiometry 1 mole of Cu form 2 moles of Ag, 2 moles of Cu form how many moles of Ag?

[tex]moles of Ag=\frac{2 moles of Cux2 moles of Ag}{1 moles of Cu}[/tex]

moles of Ag= 4 moles

4 moles of silver metal will be produced.

Mass of silver produced

The following rule of three can be applied: If by reaction stoichiometry 1 mole of Cu form 215.74 grams of Ag, 2 moles of Cu form how much mass of Ag?

[tex]mass of Ag=\frac{2 moles of Cux215.74 grams of Ag}{1 moles of Cu}[/tex]

mass of Ag= 431.48 grams

431.48 grams of silver metal will be produced.

Moles of copper (II) nitrate

The following rule of three can be applied: If by reaction stoichiometry 1 mole of Cu form 1 moles of copper (II) nitrate, 2 moles of Cu form how many moles of copper (II) nitrate?

[tex]moles of copper (II) nitrate=\frac{2 moles of Cux1 mole of copper (II) nitrate}{1 moles of Cu}[/tex]

moles of copper (II) nitrate= 2 moles

2 moles of copper (II) nitrate will be produced.

Mass of copper (II) nitrate

The following rule of three can be applied: If by reaction stoichiometry 1 mole of Cu form 187.54 grams of copper (II) nitrate, 2 moles of Cu form how much mass of copper (II) nitrate?

[tex]mass of Ag=\frac{2 moles of Cux187.54 grams of copper (II) nitrate}{1 moles of Cu}[/tex]

mass of Ag= 375.08 grams

375.08 grams of copper (II) nitrate will be produced.

Learn more about the reaction stoichiometry:

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