Question

1)Consider the following half-reactions:

Half-reaction	E° (V)
Cl2(g) + 2e- > 2Cl-(aq)	1.360V
Cd2+(aq) + 2e- > Cd(s)	-0.403V
Al3+(aq) + 3e- > Al(s)	-1.660

The strongest oxidizing agent is:

_______

enter formula

The weakest oxidizing agent is:

_______

The weakest reducing agent is:

_______

The strongest reducing agent is:

_______

Will Al³⁺(aq) reduce Cl₂(g) to Cl^-(aq)? _____yes or no

Which species can be reduced by Cd(s)? If none, leave box blank.

2) Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Cd metal is put into a 1M aqueous Cu²⁺ solution.

If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

____+____>____+____

Answer 1

The more negative dhe E, the more reducing will be agent. a strongest oxidising agent is a (chlorine) Weakest oxidising agent is 413+ weakest reducing agent is cl strongest reducing agent is Alat Since Al3t is the strongest reducing agent, it can. reduce cl to cr. Cd has a potential of -0.403 V. So it can reduce the species which has a less negative or more positive potential Therefore, cd can reduce ch to u. When cd is but in cur solution, cd should get oxidised to cd²+ & curt should get reduced to cu. cu²+ + 2e → cu 0.34V cd²+ + at → Cd -0.40u since Cd²+ has more negative potential than cuttede can reduce Cut & itself can get sedu oxidised to cal²t Balanced equation Cel + Cu²+ (d² + + cu.