Question

Consider the balanced chemical reaction Cu(s) + 2AgNO3(aq) a 2Ag(s) + Cu(NO3)2(aq)

a) Write the Complete Ionic Equation:

b) Write the Net Ionic Equation:

c) Assign oxidation numbers to all of atoms/ions in the reaction:

Cu _____ Ag _____ NO3_____ a Ag _____ Cu _____ NO3 _____

d) Which atom/ion is being oxidized in this reaction?

e) Which atom/ion is being reduced in this reaction?

Answer 1

Solution :-

Consider the balanced chemical reaction Cu(s) + 2AgNO3(aq) ------ > 2Ag(s) + Cu(NO3)2(aq)

a) Write the Complete Ionic Equation:

Cu(s) + 2Ag^+ (aq) + 2NO3^- (aq) ---- > 2Ag(s) + Cu^2+ (aq) +2 NO3^- (aq)

b) Write the Net Ionic Equation:

Cu(s) + 2Ag^+(aq)    ---- > 2Ag(s) + Cu^2+(aq)

c) Assign oxidation numbers to all of atoms/ions in the reaction:

Solution :- Oxidation states for the each element are given below the equation for the reactant side and product side on both sides the N is +5 and oxygen is -2

Cu _____ Ag _____ NO3_____ ------ > Ag _____ Cu _____ NO3 _____

0             +1          +5 -2                     0             +2          +5 -2

d) Which atom/ion is being oxidized in this reaction?

solution :- In the given reaction the Cu is changed from 0 to +2 oxidation state so the Cu(s) oxidized

e) Which atom/ion is being reduced in this reaction?

Solution :- Ag^+ is reduced to Ag(s) so the element reduced is Ag^+(aq)