Exam 20: Electrochemistry

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) Mg(s)+ Cu²⁺(aq)→ Cu(s)+ Mg²⁺(aq) Mg²⁺(aq)+ 2 e⁻ → Mg(s)E° = -2.38 V Cu²⁺(aq)+ 2 e⁻ → Cu(s)E° = +0.34 V

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ e^- → Ag(s)+ Cl^-(aq)E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0100 M and 1.55 M,respectively.The cell emf is ________ V.

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Ni and Ag⁺ in the balanced reaction? Ni(s)+ Ag⁺(aq)→ Ag(s)+ Ni²⁺(aq)

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? Ag⁺(aq)+ e⁻ → Ag(s)

Identify a component in the formation of rust.

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25°C. 2 Al(s)+ 3 Mg²⁺(aq)→ 2 Al³⁺(aq)+ 3 Mg(s)

Determine the cell notation for the redox reaction given below. Sn(s)+ 2 H⁺(aq)→ Sn²⁺(aq)+ H₂(g)

Predict the species that will be reduced first if the following mixture of molten salts undergoes electrolysis. Zn²⁺,Fe³⁺,Mg²⁺,Br^-,I^-

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I₂(s)+ Fe(s)→ Fe³⁺(aq)+ I⁻(aq)

What is the difference between a voltaic cell and an electrolytic cell?

What is the reduction half-reaction for the following overall galvanic cell reaction? Pb²⁺(aq)+ 2 Ag(s)→ Pb(s)+ 2 Ag⁺(aq)

Using the following standard reduction potentials, Fe³⁺(aq)+ e^- →Fe²⁺(aq)E° = +0.77 V Cu²⁺(aq)+ 2 e^- →Cu(s)E° = +0.34 V Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions. Cu²⁺(aq)+ 2 Fe²⁺(aq)→ 2 Fe³⁺(aq)+ Cu(s)

What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s)∣ Ba²⁺(aq) Ag⁺(aq)∣ Ag(s)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq) Cl₂(g)+ 2 e⁻ → 2 Cl⁻(aq)E° = +1.36 V Fe³⁺(aq)+ 3 e⁻ → Fe(s)E° = -0.04 V

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 2F₂(g)+ Mn(s)→ 4 F⁻(aq)+ Mn²⁺(aq) F₂(g)+ e⁻ → 2 F⁻(aq)E° = +2.87 V Mn²⁺(aq)+ 2 e⁻ → Mn(s)E° = -1.18 V

Balance the following redox reaction if it occurs in H₂SO₄.What are the coefficients in front of C₃H₈O₂ and H₂SO₄ in the balanced reaction? C₃H₈O₂(aq)+ K₂Cr₂O₇(aq)→ C₃H₄O₄(aq)+ Cr₂(SO₄)₃(aq)

What element is being oxidized in the following redox reaction? Cr(OH)₄⁻(aq)+ ClO⁻(aq)→ CrO₄^2-(aq)+ Cl⁻(aq)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. Cu(s)+ Mg²⁺(aq)→ Mg(s)+ Cu²⁺(aq) Mg²⁺(aq)+ 2 e⁻ → Mg(s)E° = -2.38 V Cu²⁺(aq)+ 2 e⁻ → Cu(s)E° = +0.34 V

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O(l) Pb(s)→ Pb²⁺(aq)+ 2 e^- How many moles of Pb(s)are oxidized by one mole of Cr₂O₇^2-?