Exam 18: Electrochemistry

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn²⁺(aq, 0.022 mol L^-1) Ag⁺(aq, 2.7 mol L^-1) ∣ Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

What is the reducing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn²⁺(aq) Ag⁺(aq) ∣ Ag(s)

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320. minutes?

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 3.20 M and [ ] = 0.000100 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

How much copper, in g, can be plated from a solution of if 3.14 A is applied for 45 minutes?

Why are iron nails coated with zinc?

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Na⁺, Ca²⁺, Cl⁻, Br⁻, F⁻

Determine the cell notation for the redox reaction given below: Sn(s) + 2Ag⁺(aq) → Sn²⁺(aq) + 2Ag(s)

Consider the galvanic cell, Which one of the following changes to the cell would cause the cell potential to increase (i.e., become more positive)?

Which of the following is the weakest oxidizing agent?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn²⁺(aq, 0.100 mol L^-1) Ag⁺(aq, 0.200 mol L^-1) ∣ Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 5.00 moles of copper metal?

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.945 M and [ ] = 1.37 M Zn(s) + (aq) → (aq) + Cr(s) E°(Zn²⁺/Zn) = -0.76 V and E°(Cr³⁺/Cr) = -0.73 V

What is the reaction at the cathode in a breathalyzer?

A voltaic cell is constructed with two -Zn electrodes, where the half-reaction is + → Zn (s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 1.17 × mol L^-1 and 8.70 × mol L^-1, respectively. The cell emf is ________ V.

Nickel can be plated from aqueous solution according to the following half-reaction. How long would it take (in min) to plate 29.6 g of nickel at 4.7 A? Ni²⁺(aq) + 2 e⁻ → Ni(s)

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s) ∣ Ni²⁺(aq) ∣∣ Cl₂(g) ∣ Cl^-(aq) ∣ C(s)

Consider the following standard reduction potentials: Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 2.00 M and [ ] = 0.00300 M Zn(s) + (aq) → (aq) + Cr(s) E°(Zn²⁺/Zn) = -0.76 V and E°(Cr³⁺/Cr) = -0.73 V

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 1.10 M and [ ] = 1.10 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V