After the chemistry lecture on single replacement redox reactions, your classmat
ID: 968420 • Letter: A
Question
After the chemistry lecture on single replacement redox reactions, your classmate tells you he has come up with a plan to produce gold and get rich. After the chemistry lecture on single replacement redox reactions, your classmate tells you he has come up with a plan to produce gold and get rich. His plan involves ordering 325.00 mL of a solution of aqueous Au(NO3)3 {gold (III) nitrate} at 0.0255 M and 13.457 g of Sn (tin) from a chemical company.
*Give the balanced molecular, ionic, and net ionic equations for a possible reaction between those two reactants including their physical states if tin has a +2 charge in the product.
*Show the balancing of the redox reaction (shown by the equation above) by separating the oxidation and reduction steps; use the net ionic equation.
Identify the oxidizing agent and the reducing agent.
*Oxidizing agent:
*Reducing agent:
*Writing the molecular equation and using an arrow show the transfer of electrons from one reactant to another
Explanation / Answer
molecular equation : 2Au(NO3)3 (aq ) + 3Sn (s)-------------------> 2Au(s) + 3Sn(NO3)2 (aq )
ionic equation : 2Au+3 (aq ) + 6NO3-(aq ) + 3 Sn (s)-------------------> 2Au (s)+ 3 Sn+2 (aq ) + 6NO3-(aq )
net ionic equation : 2Au+3 (aq ) + 3 Sn (s) ---------------------> 2 Au (s) + 3 Sn+2(aq )
oxidizing agent : 2Au(NO3)3
reducing agent : Sn
electrons flow from anode Sn to gold (Au+3)