Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question.  What is the standard cell potential (Eo), in volts, for the following voltaic cell?  Type in your answer as a number to two decimal places with no units. Al(s)|Al3+||Cr3+|Cr(s)

12. Which of the following terms can be used to describe an electrochemical cell in which a spontaneous chemical reaction generates an electric current? I. an electrolytic cell II. a galvanic cell III.  a voltaic cell 13.Which cell involves a non-spontaneous redox reaction? 14. The nickel-cadmium battery cell has a standard potential of +1.20 V. The cell reaction is 2 NiO(OH)(s) + Cd(s) + 2 H2O(l) → 2 Ni(OH)2(s) + Cd(OH)2(s). Half reactions:                    Cd(s) ------>  Cd2+ (aq)  +  2 e- 2Ni3+ (aq)  +  2e- ----->  2Ni2+ (aq)   What is the standard free energy change for this reaction? [ΔGo = -nFEocell]

Please answer the follow up question

Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter. Calculate the standard cell potential.  If the initial concentrations of Zn2+ and of OH– are 1.0 × 10–7 and 2.0 × 10–7, respectively, calculate the cell potential after the Zn2+ concentration has increased by a factor of 100. At this point, what percentage of the initial voltage remains?

Complete the half-reactions that occur at each electrode in the cell shown. Then, write the line notation for the cell. Pb -PbCl₂(s) KCl(aq) Anode half-reaction: Pb(s) + 2Cl(aq) = Cathode half-reaction: 2 AgCl(s) +2e= Pb(s) Line notation: V Cl(aq) KCl(aq) Ag PbCl₂ (s) PbCl₂(s) -AgCl(s) + 2e 2 Ag(s) + 2Cl(aq) AgCl(s) Ag(s) AgCl(s) CI (aq) CI (aq) Answer Bank 2 AgCl(s) PbCl₂ (s) 2 Ag(s) Ag(s) Pb(s) < Feedback The aqueous chloride ion is shown in the line notation in contact with the salt bridge.

1. The following oxidation and reduction half-reactions are possible for the electrolysis of potassium iodide solution. The solution contains water molecules, potassium ions (K*), and iodide ions (I-). 2H,O(1) 0,(g) + 4H*(aq) + 4e- 2H,0(1) + 2e- → H,(g) + 20H-(aq) > K*(aq) + e- -→ K(s) 21-(aq) L(s) + 2e- a. What product was formed at the anode in the electrolysis of potassium iodide solution? Explain, citing specific evi- dence from observations. your Ozg) +H* cag) +4c-→ 2 H20ee) Izca) is produced Anode the anode conforms E'eeu = + 1.23 v The product of Iz at by color change from Yellow to black Cobserved in the presence of starcn) E cell - to.SYV b. What product was formed at the cathode in the electrolysis of potassium iodide solution? Explain based on your observations. 2H20 D + le- -> Hzlg) + 20H caq) A219) $ 204- ions are ProdUced k caq) te--> K cs) E cel Hydrogen gas bubbles out fcom solution the E cel - 13 V and hv droxides turn the Phenolphthalein = - 2.93 v Solotion to pink c.…

A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X

Sketch the voltaic cell for the following reaction. Identify what is being oxidized and what is being reduced.Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+ (aq)

Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)

› Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Ni²+] = 0.00100 M and [Au³+] = 0.834 M. Standard reduction potentials can be found in this table. 3 Ni(s) + 2 Au³ +(aq) — 3 Ni² †(aq) + 2 Au(s) E = 1.72 Incorrect V