Electrochemical Cells 2

Which cell is not spontaneous?

• voltaic
• electrolytic

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

• +0.71 V
• -0.71 V

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

Calculate the standard cell potential.
Ni  + 2Fe³⁺ ---->  Ni²⁺  + 2Fe²⁺

• 1.02 V
• -1.02 V
• -0.19 V
• -0.286 V

Tags

NGSS.HS-PS3-5

Atoms of which element can most easily be oxidized?

• Copper
• Zinc
• Iron
• Calcium

Tags

NGSS.HS-PS1-2

In the electrolysis of water, hydrogen gas is produced at the 

• anode 
• cathode

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

Calculate the standard cell potential cell in the following:
Zn / Zn²⁺ // Pb²⁺ / Pb

• +0.89 V
• + 0.63 V
• - 0.89 V
• - 0.63 V

A galvanic cell was set up using the Cu²⁺/Cu and Fe³⁺/Fe²⁺ half-cells. The standard reduction 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 oxidizing and reducing agents in this galvanic cell are, respectively:   

• Fe³⁺; Cu
• Fe²⁺; Cu
• Cu²⁺; Fe³⁺
• Cu²⁺; Fe²⁺

Tags

NGSS.HS-PS1-2

The net products that result from the electrolysis of water are?

• H₂ and OH^-
• O and H⁺
• H⁺ and OH^-
• H₂ and O₂

The electrolysis of molten sodium chloride produces:

• hydrochloric acid
• sodium metal and chlorine gas
• chlorine gas and aqueous sodium hydroxide
• glucose

Tags

NGSS.HS-PS3-5