Electrochemistry 2

Calculate standard cell potential for this equation:

Zn²⁺(aq) + 2e → Zn(s) Eº = – 0.76 V

Cd²⁺(aq) + 2e → Cd(s) Eº = – 0.40 V

• E^ocell = -0.36 V

• E^ocell = -1.16 V

• E^ocell = +1.16 V

• E^ocell = +0.36 V

Which is correct to write cell notation

Anode: Zn

Cathode: Ni

• Zn²⁺ (aq,1M) / Zn (s) // Ni (s) / Ni²⁺ (aq,1M)

• Zn (s) /Zn²⁺ (aq,1M) // Ni²⁺ (aq,1M) / Ni (s)

• Zn²⁺ (s,1M) / Zn (aq) // Ni (aq) / Ni²⁺ (s,1M)

• Zn (aq) /Zn²⁺ (s,1M) // Ni²⁺ (s,1M) / Ni (aq)

Which of the species strong oxidizing agent?

Cl₂(g) + 2e → 2Cl^-(aq) E^ocell = + 1.36 V

Cu²⁺(aq) + 2e → Cu(s) E^ocell = + 0.34 V

Ni²⁺(aq) + 2e → Ni(s) E^ocell = – 0.25 V

Ca²⁺(aq) + 2e → Ca(s) E^ocell = – 2.87 V

• Cl₂(g)

• Cu²⁺(aq)

• Ni²⁺(aq)

• Ca²⁺(aq)

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu²⁺/Cu = 0.34V

Zn²⁺/Zn = -0.76V

• Cu

• Zn

• CuSO4

• ZnSO4

In the following reaction

Sn⁺² + 2Fe⁺³ --> Sn⁺⁴ + 2Fe⁺²,

the reducing agent is...

• Fe⁺³

• Sn⁺²

• Sn⁺⁴

• Fe⁺²

Tags

NGSS.HS-PS1-2

What is oxidation number of Cr in Cr₂O₇^2-?

• -2

• +2

• +6

• +12

Tags

NGSS.HS-PS1-1

Calculate standard cell potential for this equation:

Zn²⁺(aq) + 2e → Zn(s) Eº = – 0.76 V

Cd²⁺(aq) + 2e → Cd(s) Eº = – 0.40 V

• E^ocell = -0.36 V

• E^ocell = -1.16 V

• E^ocell = +1.16 V

• E^ocell = +0.36 V

What is the oxidation number of nitrogen in N₂?

• -3

• 0

• +4

• -1

Which element is oxidised in the reaction Zn + 2HCl  $\rightarrow$   ZnCl2 + H2 $\$ 

• Zinc
  

• Hydrogen

• Chlorine

• None

What are the coefficients when the equation is balanced?

• 1 + 1 + 1 --> 2 + 1 + 3
• 2 + 2 + 2 --> 4 + 2 + 3
• 1 + 2 + 1 --> 2 + 2 + 3
• 1 + 1 + 1 --> 1 + 1 + 1

Tags

NGSS.HS-PS1-7