Use the References to access important values if needed for this question. Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: 2Cr+ (aq) + 3Co(s) → 2Cr(s) + 3C02+ (aq) Answer: kJ K for this reaction would be than one. greater less Retry Entir 2 more group attempts remaining Submit Answer

Use the References to access important values if needed for this question. Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: 2Cr+ (aq) + 3Co(s) → 2Cr(s) + 3C02+ (aq) Answer: kJ K for this reaction would be than one. greater less Retry Entir 2 more group attempts remaining Submit Answer

Chemistry

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Chapter18: Electrochemistry

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Problem 119AE: The black silver sulfide discoloration of silverware can be removed by heating the silver article in...

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Electrolysis of a solution of CuSO4(aq) to give copper metal is carried out using a current of 0.66 A. How long should electrolysis continue to produce 0.50 g of copper?
What volume of F2 gas, at 25C and 1.00 atm, is produced when molten KF is electrolyzed by a current of 10.0 A for 2.00 h? What mass of potassium metal is produced? At which electrode does each reaction occur?
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)?
The black silver sulfide discoloration of silverware can be removed by heating the silver article in a sodium carbonate solution in an aluminum pan. The reaction is 3Ag2S(s)+2Al(s)6Ag(s)+3S2(aq)+2Al3+(aq) a. Using data in Appendix 4, calculate G, K, and for the above reaction at 25C. [For Al3+(aq), Gf = 480. kJ/mol.] b. Calculate the value of the standard reduction potential for the following half-reaction: 2e+Ag2S(s)2Ag(s)+S2(aq)
Identify the reaction at the anode, reaction at the cathode, the overall reaction, and the approximate potential required for the electrolysis of the following molten salts. Assume standard states and that the standard reduction potentials in Appendix L are the same as those at each of the melting points. Assume the efficiency is 100%. (a) CaCl2. (b) LiH. (c) AlCl3. (d) CrBr3
Consider the electrolysis of NiCl2 to Ni(s) and Cl2(g). (a) What is the minimum voltage required to carry out this reaction at standard conditions? (b) If a voltage of 3.0 V is actually used, and 10.00 kJ of energy are consumed, how many grams of Ni(s) are obtained? (1J=1volt-coulomb)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
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.
Consider the following cell reaction at 25C. 2Cr3+(aq)+3Zn(s)3Zn2(aq)+2Cr(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain G for the cell reaction. Use data in Appendix C to calculate H; note that Cr(H2O)63+(aq) equals Cr3+(aq). Use these values of H and G to obtain S for the cell reaction.

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