Question

Which species functions as the oxidizing agent in the following reduction-oxidation reaction?

Which one the reducing agent?
Which one is oxidized?
Which one is reduced?
Which one loses electrons?
Which one gains electrons?
Zn(s) + Cu2+(aq) ? Cu(s) + Zn2+(aq).

Answer 1

See explanation

Step-by-step explanation:

In this case, we can start with the half-reactions. If the total reaction is:

`Zn_(_s_)~+~Cu^2^+~_(_a_q_)~->~Cu_(_s_)~+~Zn^2^+_(_a_q_)`

If we split the reaction we will have:

Half-reaction 1:

`Zn_(_s_)~->~Zn^2^+_(_a_q_)`

Half-reaction 2:

`Cu^2^+~_(_a_q_)~->~Cu_(_s_)`

Now we can add the electrons, keeping in mind that we have to obtain zero charge in both sides of each half-reaction:

Half-reaction 1:

`Zn_(_s_)~->~Zn^2^+_(_a_q_)~+~2e^-`

Half-reaction 2:

`Cu^2^+~_(_a_q_)~+~2e^-~->~Cu_(_s_)`

With this in mind, we can solve the questions:

Which one loses electrons?

In half-reaction number 1 we have the electrons in the products side, therefore this half-reaction is the one that loses electrons.

Which one gains electrons

In half-reaction number 2 we have the electrons in the reagent side, therefore this half-reaction is the one that gains electrons.

Which one is oxidized?

If half-reaction number 1 loses electrons will be the oxidation reaction.

Which one is reduced?

If half-reaction number 2 gains electrons will be the reduction reaction.

Which species functions as the oxidizing agent in the following reduction-oxidation reaction?

If half-reaction number 2 is the reduction will be a oxidizing agent.

Which one the reducing agent?

If half-reaction number 1 is the oxidation will be a reducing agent.

I hope it helps!