Question

Part A

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 MnO₄^–(aq),Mn²⁺(aq), and H⁺(aq)

Which of the following statements match the cathode?

Select all that apply.

Group of answer choices

The electrode increases in mass

Oxidation occurs at this half-cell

Electrons enter the half-cell

The electrode is inactive

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

The electrode is negative

Part B

Which of the following are always true for a voltaic cell?

Select all that apply.

Group of answer choices

Electrons flow from anode to cathode

Anions flow to the anode

A spontaneous reaction occurs

The anode electrode loses mass

None of the above

Part C

Fill in the blanks:

In a voltaic cell a   ["spontaneous", "nonspontaneous"]         reaction occurs, therefore this cell ["requires energy", "can supply energy"]         .

Answer 1

Part A

In a voltaic cell, The negative electrode that is cathode increases in mass,

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

The electrode is negative and reduction occurs at the negative electrode

Part B

In a voltaic cell,

Electron flow from anode to cathode which was released when Zn gets oxidised to Zn²⁺ and that electrons move to the cathode.

Anions doesn't move to the anode as Zinc electrode is acting as anode so it gets oxidised to form Zn²⁺ which remains in the electrolyte and electrons which were released during this half cell reaction were move from the anode to the cathode.

A spontaneous reaction is responsible for the electricity to generate from this voltaic cell.

During electrolysis , oxidation occurs at anode during which solid metal atoms changes into ions as they lose electrons . Therefore,as loss of mass occurs at anode its mass is decreasing.

Part C

In a voltaic cell a spontaneous reaction occurs, therefore this cell can supply energy for generating electricity.