Question

MAXIMUM POINTS!! PLEASE HELP!

If copper metal pieces were added to an aqueous solution of silver nitrate, the Silver would be replaced in a single replacement reaction forming aqueous copper (II) nitrate and solid silver.

1. Write a balanced chemical equation for the reaction.


2. How much silver is produced is 15.00 grams of Cu is added to the solution of excess silver nitrate?


3. If silver metal sells for $4.50/ounce, how much would the Silver collected be worth? (1 gram = 0.0353 oz)

Answer 1

1.The balanced chemical equation is as below

Cu + 2 Ag(NO)₃ → Cu(NO₃)₂ +2 Ag

2.The much silver produced is 50.9 g

Step 1: find the moles of Cu

moles = mass÷ molar mass

from periodic table the molar mass of Cu = 63.5 g/mol

moles is therefore = 15.00 g÷ 63.5 g/mol = 0.236 moles

Step 2: use the mole ratio to determine the moles of Ag

from equation above Cu:Ag is 1:2

therefore the moles of Ag =0.236 moles x 2/1 =0.472 moles

Step 3: find the mass of Ag

mass = moles x molar mass

from periodic table the molar mass of Ag =107.87 g/mol

mass = 0.472 moles x 107.87 g/mol = 50.9 g

3. The much silver collected worth is 1.797 oz

convert 50.9 g to oz

that is 1 gram = 0.0353 oz

50.9 grams =? oz

by cross multiplication

={(50.9 grams x 0.0353 oz) / 1 gram} =1.797 oz