Using the following data, calculate the standard standard cell potential for an cell based on the reaction below, and tell whether the reaction is electrochemical spontaneous. Cr (s) + 3Fe³+ (aq) Half-reaction Cr3+ (aq) + 3e¯ → Cr (s) Fe2+ (aq) + 2e →→ Fe (s) - 3Fe2+ (aq) + Cr3+ (aq) Fe³+ (aq) + e → Fe²+ (s) Sn4+ (aq) + 2e Sn²+ (aq) 2+ (A) -1.45 V, spontaneous (B) -1.51 V not spontaneous (C) 2.99 spontaneous (D) +1.51 spontaneous E° (V) -0.74 -0.440 +0.771 +0.154

Using the following data, calculate the standard standard cell potential for an cell based on the reaction below, and tell whether the reaction is electrochemical spontaneous. Cr (s) + 3Fe³+ (aq) Half-reaction Cr3+ (aq) + 3e¯ → Cr (s) Fe2+ (aq) + 2e →→ Fe (s) - 3Fe2+ (aq) + Cr3+ (aq) Fe³+ (aq) + e → Fe²+ (s) Sn4+ (aq) + 2e Sn²+ (aq) 2+ (A) -1.45 V, spontaneous (B) -1.51 V not spontaneous (C) 2.99 spontaneous (D) +1.51 spontaneous E° (V) -0.74 -0.440 +0.771 +0.154

Chemistry

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 150CP: Given the following two standard reduction potentials, solve for the standard reduction potential of...

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Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?
An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)

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