Answer:
1.3710 grams of silver metal can be formed.
0.4158 grams of the excess reactant will be left over when the reaction is complete
Explanation:
Moles of zinc metal =
Moles of silver nitrate =
According to reaction , 1 mole of zinc reacts with 2 mole of silver nitrate.
Then 0.0864 mol of zinc will react with:
silver nitrate
This means that zinc is in excessive amount.
So, the formation of silver metal will depend on moles of silver nitrate.
According to reaction 2 moles of silver nitrate produces 2 mole of silver metal.
Then 0.01271 moles of silver nitrate will produce:
of silver metal
Mass of 0.01271 mol of silver metal = 0.01271 mol × 107.87 g/mol = 1.3710 g
Moles of excessive reagent left
According to reaction , 1 mole of zinc reacts with 2 mole of silver nitrate.
Then 0.01271 mol of silver nitrate will react with:
of zinc
Moles of an excess reagent = 0.01271 mol - 0.00635 mol = 0.00636 mol
Mass of 0.00636 mol zinc:
0.00636 mol × 65.38 g/mol = 0.4158 g
1.3710 grams of silver metal can be formed.
0.4158 grams of the excess reactant will be left over when the reaction is complete