Electrochemistry MCQ 2

The standard reduction potential of metals A,B,C and D are -0.40v, +0.34v,+0.8v and -1.67v. The metal that can displace all others is

• D

• B

• A

• C

Cu∣Cu2+∥Fe2+,Fe3+∣Pt In this cell

• Copper ion is the oxidizing agent

• Copper is the oxidizing agent

• Fe3+ is the oxidizing agent

• Fe2+ is the oxidizing agent

The standard reduction potential value of the three metallic cations X, Y and Z are 0.52, -3.03 and -1.18 V respectively. the order of reducing power of the corresponding metals is

• Y>X>Z

• X>Y>Z

• X>Z>Y

• Y>Z>X

Which of the following will form the cathode with respect to iron anode in an electrolyte cell - ( Eo = - 0.40 v)

• Mg ( - 2.37v)

• Cd (- 0.44v)

• Ni (- 0.22v)

• Al (-1.67v)

A cell constructed by coupling copper and magnesium electrode has emf of 2.7 volts. if the standard reduction potential of copper electrode is +0.34 volts, that of magnesium electrode is

• 2.36v

• -3.04v

• +3.04

• -2.36v

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

Tags

NGSS.HS-PS1-2

Which metal is the negative electrode?

Zn/Zn²⁺ // Cu²⁺/Cu

• zinc

• copper

Tags

NGSS.HS-PS1-1

What reaction occurs at the anode?

Ag⁺/Ag = 0.80V

Ni²⁺/Ni = -0.25V

• Ag⁺ + e^- →Ag

• Ag → Ag⁺ + e^-

• Ni²⁺ + 2e^- → Ni

• Ni → Ni²⁺ + 2e^-

Tags

NGSS.HS-PS1-2

What would be the theoretical cell potential of the previous electrochemical cell?

Ag⁺/Ag = 0.80V

Ni²⁺/Ni = -0.25V

• 1.05V

• -1.05V

• 0.55V

• -0.55V

Given the standard electrode potentials,

K+/K = −2.93V, Ag+/Ag = 0.80V,

Hg2+/Hg = 0.79V

Mg2+/Mg = −2.37 V, Cr3+/Cr = − 0.74V

their increasing order of reducing power.

• K<Mg<Cr<Hg<Ag

• Ag >Hg > Cr > Mg > K

• Ag < Hg < Cr < Mg < K

• K>Mg>Cr>Hg>Ag