Exam 18: Electrochemistry

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Cd and Ag⁺ in the balanced reaction? Cd(s)+ Ag⁺(aq)→ Ag(s)+ Cd²⁺(aq)

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

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 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

Which of the following is the strongest reducing agent?

What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s)∣ Fe³⁺(aq)∣∣ Cl₂(g)∣ Cl⁻(aq)∣ Pt

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K)for the following balanced redox reaction at 25°C. Pb²⁺(aq)+ Cu(s)→ Pb(s)+ Cu²⁺(aq)

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s)+ Cu(NO₃)₂(aq)→ Pb(NO₃)₂(aq)+ Cu(s)

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ · xH₂O The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

Which of the following reactions would have the smallest value of K at 298 K?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Fe²⁺(aq)+ K(s)→ Fe(s)+ K⁺(aq)

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s)∣ Zn²⁺(aq)∣∣ Ni²⁺(aq)∣ Ni(s)

Using the following standard reduction potentials, Fe³⁺(aq)+ e^- → Fe²⁺(aq)E° = +0.77 V Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 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. Ni²⁺(aq)+ 2 Fe²⁺(aq)→ 2 Fe³⁺(aq)+ Ni(s)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s)∣ Al³⁺(aq,0.115 M)∣∣ Al³⁺(aq,3.89 M)∣ Al(s)

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 three moles of Cr₂O₇^2-?

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

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Al and F₂ in the balanced reaction? Al(s)+ F₂(g)→ Al³⁺(aq)+ F^-(aq)

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