Question

Each of the following reactions involves a transfer of electrons. The number of electrons transferred is represented with the letter n . For each of the following balanced reactions, determine the number of electrons transferred.

Part A

2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)

Express your answer using an integer.

Part B

Consider a voltaic cell that is set up as follows:

Anode contains an Fe(s) electrode and 1M Fe²⁺(aq)

Cathode contains a Ni(s) electrode and 1M Ni²⁺(aq)

Which of the following statements match the anode?

The electrode is negative

Electrons enter the half-cell

The electrode decreases in mass

The electrode is inactive

Oxidation occurs at this half-cell

Cations from the salt-bridge move to this half-cell

Part C

Consider a voltaic cell that is set up as follows:

Anode contains an Zn(s) electrode and 1M Zn²⁺(aq)

Cathode contains a Pt(s) electrode and 1M MnO_4^–(aq),Mn²⁺(aq), and H⁺(aq)

Which of the following statements match the cathode?

Cations from the salt-bridge move to this half-cell

Electrons enter the half-cell

Oxidation occurs at this half-cell

The electrode is inactive

The electrode increases in mass

The electrode is negative

Answer 1

Part A

2Fe³⁺(aq)+3Sn(s)→2Fe(s)+3Sn²⁺(aq)

Oxidation state of Fe changes from +3 to 0 so, it gains 3 electrons

Oxidation state of Sn changes from 0 to +2 so it loses 2 electrons

In the overall balanced equation, 6 electrons are transferred.

PART(B)

* The electrode is negative

* The electrode decreases in mass

* Oxidation occurs at this half cell

PART(C)

* Cations from the salt bridge move to this half cell

* Electrons enter the half cell

* The electrode is inactive

* The electrode increases in mass