11ElectrochemistryPracticeTest

Which of the following is the correct cell notation for the reaction

Hg₂²⁺ + Cd(s) → Cd²⁺ + 2Hg(l)

• Cd²⁺ | Cd | | Hg₂²⁺ | Hg

• Cd²⁺ | Hg₂²⁺ | | Cd | Hg

• Cd | Cd²⁺ | | Hg₂²⁺ | Hg

• Cd²⁺ | Hg | | Hg₂²⁺ | Cd

• Hg | Cd | | Hg₂²⁺ | Cd²⁺

Consider an electrochemical cell where the following reaction takes place:

3Sn²⁺(aq) + 2Al(s) → 3Sn(s) + 2Al³⁺(aq)

Which of the following is the correct cell notation for this cell?

• Al | Al³⁺ | | Sn²⁺ | Sn

• Al³⁺ | Al | | Sn | Sn²⁺

• Sn | Sn²⁺ | | Al³⁺ | Al

• Sn | Al³⁺ | | Al | Sn²⁺

• Al | Sn²⁺ | | Sn | Al³⁺

An early method of producing aluminum metal was the reaction of aluminum salts with sodium metal:

Al³⁺ + 3Na(s) ↔ Al(s) + 3Na⁺ E° = +1.05 V

What is ΔG° for this reaction

• -304 kJ

• -101 kJ

• +101 kJ

• +202 kJ

• +304 kJ

Calculate ΔG for the following reaction:

I₂(s) + 2Br^-(aq) → 2I^-(aq) + Br₂(l)

• +105 kJ

• -105 kJ

• +312 kJ

• +52 kJ

• -312 kJ

If ΔG of the following reaction is -203 kJ, what is E°?

2Ag⁺(aq) + Ni(s) → 2Ag(s) + Ni²⁺(aq)

• -1.05 V

• +2.10 V

• +0.0011 V

• -0.011 V

• +1.05 V

Given the two half reactions and their potentials, which net reaction is spontaneous?

Mg²⁺(aq) + 2e^- → Mg(s) E° = -2.37 V

Ni²⁺(aq) + 2e^- → Ni(s) E° = -0.25 V

• Ni(s) + Mg²⁺(aq) → Mg(s) + Ni²⁺(aq)

• Ni²⁺(aq) + Mg(s) → Mg²⁺(aq) + Ni(s)

• Ni(s) + Mg(s) → Mg²⁺(aq) + Ni²⁺(aq)

• Mg²⁺(aq) + Ni²⁺(aq) → Mg(s) + Ni(s)

• Mg²⁺(aq) + Mg(s) → Ni(s) + Ni²⁺(aq)

Calculate E° for the following reaction:

Sn⁴⁺(aq) + 2K(s) → Sn²⁺(aq) + 2K⁺(aq)

• +6.00 V

• -3.08 V

• +3.08 V

• +2.78 V

• -2.78 V

Calculate E° for the following reaction:

2Al³⁺(aq) + 3Cd(s) → 2Al(s) + 3Cd²⁺(aq)

• -2.06 V

• +4.52 V

• +2.06 V

• -4.52 V

• -1.26 V

Using data from the reduction potential table and the reaction

2Ag(s) + Pt²⁺(aq) → Pt(s) + 2Ag⁺(aq) E° = 0.38 V

calculate the standard reduction potential of the half-reaction

Pt²⁺(aq) + 2e^- → Pt(s)

• -1.18 V

• -0.40 V

• 0.40 V

• 1.18 V

• 2.00 V

An electrochemical cell of notation Pd | Pd²⁺ | | Cu²⁺ | Cu has an E° = -0.65 V. If we know that the standard reduction potential of Cu²⁺/Cu is E° = 0.34 V, what is the standard reduction potential for Pd²⁺/Pd?

• -0.99 V

• -0.31 V

• +0.31 V

• 0.62 V

• +0.99 V