Galvanic Cells - Assessment

Galvanic Cells

Assessment

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Nena Zee

•

Chemistry

•

11th - 12th Grade

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28 questions

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Multiple Choice

1 min

1 pt

In a Galvanic Cell, the anode is...

positive

negative

Multiple Choice

30 sec

1 pt

In a Galvanic Cell, the cathode is...

positive

negative

Multiple Choice

30 sec

1 pt

Oxidation occurs at the...

anode

cathode

Multiple Choice

1 min

1 pt

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

anode to the cathode

cathode to the anode

Multiple Choice

30 sec

1 pt

E_cell =

E_red - E_ox

E_red + E_ox

E_ox - E_red

E_ox + E_red

Multiple Choice

30 sec

1 pt

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

Cu | Cu²⁺

Zn | Zn²⁺

Multiple Choice

30 sec

1 pt

In any Galvanic Cell, which half cell will undergo reduction?

The half cell with the lower standard electrode potential

The half cell with the higher standard electrode potential

Multiple Choice

30 sec

1 pt

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

Multiple Choice

30 sec

1 pt

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

10.

Multiple Select

1 min

1 pt

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

is oxidised

is reduced

increases its oxidation number

decreases its oxidation number

11.

Multiple Select

30 sec

1 pt

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

is oxidised

is reduced

increases its oxidation number

decreases its oxidation number

12.

Multiple Choice

1 min

1 pt

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

13.

Multiple Choice

30 sec

1 pt

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

positive

negative

14.

Multiple Choice

1 min

1 pt

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.

15.

Multiple Choice

30 sec

1 pt

What is the standard electrode which all other standard electrode potentials are measured against?

helium

hydrogen

magnesium

potassium

16.

Multiple Choice

1 min

1 pt

A VCE chemistry student sets up a galvanic cell using two standard half-cells with half reactions.
Half-cell 1: Cr³⁺(aq)+e^-→Cr²⁺(aq)
Half-cell 2: Cr(s)→Cr²⁺(aq)+2e^-Sutable materials for the electrodes of te two half-cells are

Half-cell 1: Platinum; Half-cell 2: Platinum

Half-cell 1: Platinum; Half-cell 2: Chromium

Half-cell 1: Chromium; Half-cell 2: Chromium

Half-cell 1: Chromium; Half-cell 2: Platinum

17.

Multiple Choice

1 min

1 pt

Reactions in galvanic cells are

spontaneous, redox reactions

non-spontaneous, redox reactions

spontaneous, non-redox reactions

non-spontaneous, non-redox reactions

18.

Multiple Choice

1 min

1 pt

In the wet corrosion of iron, iron is oxidised, while ________ is reduced.

Oxygen

Water

Hydrogen

Iron (III)

19.

Multiple Choice

2 mins

1 pt

A VCE chemistry student sets up a galvanic cell using two standard half-cells with half reactions.

Half-cell 1: Cr³⁺(aq)+e^-→Cr²⁺(aq)

Half-cell 2: Cr(s)→Cr²⁺(aq)+2e^-

Using this information, we can determine that;

Half-cell 1 is the anode, where oxidation occurs

Half-cell 1 is the cathode, where reduction occurs

No spontatneous reaction will occur, since only chromium is involved

Cr³⁺is the reductant, since it undergoes reduction

20.

Multiple Choice

5 mins

1 pt

A galvanic cell consists of one half-cell that is made up of an inert graphite electrode in a solution containing 1.0 M Fe²⁺ (aq) and 1.0 M Fe³⁺ (aq) at 25^oC. Which one of the following could be used as the second half-cell so that the polarity of the electrode in this second half-cell is positive?

a lead electrode in a solution of 1.0 M Pb²⁺ (aq)

a silver electrode in a solution of 1.0 M Ag⁺ (aq)

an iron electrode in a solution of 1.0 M Fe²⁺ (aq)

an inert graphite electrode in a solution of 1.0 M Br^- (aq)

21.

Multiple Choice

45 sec

1 pt

What is oxidation number of Cr in Cr₂O_7^2-?

-2

+12

22.

Multiple Choice

45 sec

1 pt

Which are examples of reduction?

I and II

I and III

II and III

I, II and III

23.

Multiple Choice

1 min

1 pt

Which energy conversion shown below takes place in an electrochemical cell?

Electrical to chemical

Mechanical to chemical

Mechanical to electrical

Chemical to electrical

24.

Multiple Choice

30 sec

1 pt

If in a reaction, copper is reduced; its number of electrons has:

Increased

Decreased

Remained Constant

Varies Randomly

25.

Multiple Choice

30 sec

1 pt

Calculate the standard cell potential.
3Mg + 2Al³⁺ --> 2Al + 3Mg²⁺

+0.71 V

-0.71 V

26.

Multiple Choice

1 min

1 pt

If the cell potential is negative, the reaction is?

a success

spontaneous

not spontaneous

27.

Multiple Choice

5 mins

1 pt

Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, E^o, for the following reactions. Both cells generate a potential difference.
Ag(NH₃)₂⁺(aq) + e^-↔ Ag(s) + 2NH₃(aq); E^o₁
Ag⁺(aq) + e^-↔ Ag(s); E^o₂Ag(CN)^-₂(aq) + e^-↔ Ag(s) + 2CN^- (aq); E^o₃
The values of the electrode potentials in order from highest to lowest would be

E^o_1;E^o_2;E^o₃

E^o_1;E^o₃; E^o₂

E^o₂;E^o_1;E^o₃

E^o₃; E^o₂;E^o₁

28.

Multiple Choice

3 mins

1 pt

What reaction occurs at the anode?

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni²⁺ + 2e^- → Ni

Ni → Ni²⁺ + 2e^-

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