Redox 1: Galvanic Cells

Consider the galvanic cell given.
Which of the following deductions about this cell is correct?

• Oxidation is occurring in half-cell 2
• The positive electrode is in half-cell 2
• Oxidation is occurring in half-cell 1
• The negative electrode is in half-cell 1

Tags

NGSS.HS-PS2-5

Consider the galvanic cell represented, operating at 25^oC , 101.3 kPa and using 1 M solutions. 
The product(s) of the half-reaction occurring in half-cell 1 is (are)

• Ni (s)
• Ni²⁺ (aq)
• H₂O₂ (aq)/H⁺ (aq)
• H₂O (l)

Tags

NGSS.HS-PS1-2

A galvanic cell is established to power a torch, as shown.
For this cell, the

• electrons will flow from the aluminium to the hydrogen half-cell
• aluminium electrode will be the positive anode
• concentration of aluminium ions in solution will be falling
• hydrogen half-cell will be the negative cathode

Tags

NGSS.HS-PS1-2

A galvanic cell is established to power a torch, as shown.
For this cell, the overall equation will be

• 2Al(s)+3H_2(g)→2Al³⁺(aq)+6H⁺(aq)
• 3Cl^-(aq)+Al(s)→AlCl₃(aq)
• 2Al³⁺(aq)+3H_2(g)→2Al(s)+6H⁺(aq)
• 2Al(s)+6H⁺(aq)→2Al³⁺(aq)+3H₂(g)

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-4

NGSS.HS-PS1-7

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

The experimental arrangement shows a:
- silver rod dipping into a 1.0 M solution of AgNO₃ (aq)
- nickel rod dipping into a 1.0 M solution of Ni(NO₃)₂ (aq)
The solutions are connected to each other with a salt bridge consisting of an inverted U-tube containing ammonium nitrate solution.
Which of the following alternatives correctly describes the polarity of, and the reaction that occurs at, the anode of this cell?

• Negative; Ag⁺(aq)+e^-→Ag(s)
• Negative; Ni(s)→Ni²⁺(aq)+2e^-
• Positive; Ag⁺(aq)+e^-→Ag(s)
• Positive; Ni(s)→Ni²⁺(aq)+2e^-

Tags

NGSS.HS-PS1-2

NGSS.HS-PS2-5

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)

Tags

NGSS.HS-PS3-5

Two standard galvanic cells are shown.
On the basis of the polarity of the electrodes shown, which one of the following reactions would NOT be expected to occur spontaneously?

• Co²⁺(aq)+Cd(s)→Co(s)+Cd²⁺(aq)
• 2Mn³⁺(aq)+Co(s)→2Mn²⁺(aq)+Co²⁺(aq)
• 2Mn³⁺(aq)+Cd(s)→2Mn²⁺(aq)+Cd²⁺(aq)
• 2Mn²⁺(aq)+Co²⁺(aq)→2Mn³⁺(aq)+Co(s)

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-4

NGSS.HS-PS3-1

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^o₂
Ag(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

Tags

NGSS.HS-PS3-1