Free Printable Galvanic Cells

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Galvanic Cells

Total questions: 22

Worksheet time: 37mins

Name

Class

Date

In a Galvanic Cell, the anode is...

positive

negative

In a Galvanic Cell, the cathode is...

positive

negative

Oxidation occurs at the...

anode

cathode

Reduction occurs at the...

anode

cathode

E_cell =

E_red - E_ox

E_red + E_ox

E_ox - E_red

E_ox + E_red

In a Galvanic cell, the electrons flow from the...

anode to the cathode

cathode to the anode

In a Galvanic Cell, the salt bridge...

completes the circuit so that electrons can flow through the wire

maintains charge balance

is soaked in an unreactive electrolyte such as KNO₃

all of the above

In the above Galvanic Cell, which half cell is undergoing reduction?

Cu | Cu²⁺

Zn | Zn²⁺

If an electrochemical reaction is spontaneous, what will E_cell be?

positive

negative

10.

Consider the galvanic cell reaction Zn (s) + Cu²⁺ (aq) → Cu (s) + Zn²⁺ (aq) When the cell is running spontaneously, which is the only true statement?

The copper electrode loses mass and the zinc electrode is the cathode.

The copper electrode gains mass and the copper electrode is the cathode.

The zinc electrode gains mass and the zinc electrode is the anode.

The zinc electrode loses mass and the zinc electrode is the cathode.

11.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the anode?

HgO + 2 e- → Hg + O^2-

Zn²⁺ + 2 e- → Zn

Zn → Zn²⁺ + 2 e-

ZnO + 2 e- → Zn

12.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the cathode?

HgO + 2 e- → Hg + O^2-

Hg → Hg²⁺ + 2 e-

Zn → Zn²⁺ + 2 e-

ZnO + 2 e- → Zn

13.

In a redox reaction, the oxidising agent... (choose two options)

is oxidised

is reduced

increases its oxidation number

decreases its oxidation number

14.

A galvanic cell was set up using the Cu²⁺/Cu and Fe³⁺/Fe half-cells. The standard redox potentials for these half-cells are:
Cu²⁺(aq) + 2e^- → Cu(s); E⁰ = 0.34 V
Fe³⁺(aq) + e^- → Fe²⁺(aq); E⁰ = 0.77 V
The oxidant and reductant reacting in this galvanic cell are, respectively:

Fe³⁺; Cu

Fe²⁺; Cu

Cu²⁺; Fe³⁺

Cu²⁺; Fe²⁺

15.

A galvanic cell was set up from a Cl₂/Cl^- half-cell and a standard hydrogen electrode (SHE). It was found that the voltmeter reading was 1.36 V and the chlorine half-cell was the positively-charged electrode. Which statement about this galvanic cell is INCORRECT?

Both of the electrodes should be made of platinum.

The chlorine half-cell is the anode.

As the cell operates, the pH of the solution in the SHE decreases.

The standard redox potential for the chlorine half-cell must be +1.36 V.

16.

A galvanic cell was set up using the Pb⁴⁺/Pb²⁺ and Pb²⁺/Pb half-cells. The standard redox potentials for these half-cells are:
Pb⁴⁺(aq) + 2e^- → Pb²⁺(aq); E⁰ = 1.69 V
Pb²⁺(aq) + e^- → Pb(s); E⁰ = -0.13 V
What metal should be used for the electrode for the Pb⁴⁺/Pb²⁺ half-cell and what would be the potential difference across the cell?

Lead; 1.56 V

Lead; 1.82 V

Platinum; 1.56 V

Platinum; 1.82 V

17.

Calculate the cell potential of voltaic cell

–1.51

- 0.03

+0.03

+1.51

18.

Voltaic cell is made by connecting two half-cells below. Which statement is correct?

Mn is oxidized and voltage is 1.06 V

Pb is oxidized and voltage is 1.06 V

Mn is oxidized and voltage is 1.32 V

Pb is oxidized and voltage is 1.32 V

19.

As an element is oxidized, its oxidation number

decreases as electrons are lost

increases as electrons are lost

decreases as electrons are gained

increases as electrons are gained

20.

What reaction occurs at the anode?

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni²⁺ + 2e^- → Ni

Ni → Ni²⁺ + 2e^-

21.

Reduction happens at the

anode

cathode

salt bridge

voltmeter

22.

This electrode loses mass

anode

cathode

Reset

Galvanic Cells

Total questions: 22

Worksheet time: 37mins

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