How many grams of nickel metal will be deposited from a solution that contains Ni²* ions if a current of 0.704 A is applied for 67.7 minutes.grams Standard Reduction (Electrode) Potentials at 25 °CStandard Reduction (Electrode) Potentials at 25 °CHalf-ell ReactionE (volts)Half-Cell Reaction(volts)Cr"(aq) + 3 e Cr[s)Za"(aq) + 2 e-Zn[s)-0.74F2(8) + 2 e2 F'(aq)2.87-0.763Ce* (aq) + e' Ce³*(aq)Mno, (aq) + 8 H"(aq) + 5 e Mn²"(aq) + 4 H,0(1)1.612 H,0() + 2 e-Hz(R) + 2 OH (aq)-0.831.51Mn2"(aq) + 2 e- Mn(s)-1.18Cl2(8) + 2 e 2 cI(aq)1.36A"(aq) + 3 e→Al(s)-1.66Cr20, (aq) + 14 H'(aq) + 6 e' →2 Cr*"(aq) + 7 H20(1)1.33Mg2"(aq) + 2 e- Mg(s)-2.3702(8) + 4 H"(aq) + 4 e2 H20(1)1.229Na"(aq) + e Na(s)-2.714Brz(1) + 2 e 2 Br'(aq)K"(aq) +e K(s)-2.9251.08NO, (aq) + 4 H"(aq) + 3 e NO(g) + 2 H,0)Li (aq) + eLi(s)-3.0450.962 Hg2 (aq) + 2 e - Hg,"(aq)0.920Hg"(aq) + 2 e- Hg(1)0.855Ag"(aq) + e Ag(s)0.799Hg,"(aq) + 2 e–2 Hg()0.789Fe"(aq) + eFe²"(aq)0.77112(8) + 2 e2 I(aq)0.535Fe(CN), (aq) + e' Fe(CN),*(aq)0.48Cu2 (aq) + 2 e →Cu(s)0.337Cu"(aq) + e Cu"(aq)0.153S(s) + 2 H"(aq) + 2 e H,S(aq)0.142 H"(aq) + 2 e- H2(8)0.0000Ph (aq) + 2 e' Ph(s)-0.126Sn2*(aq) + 2 e- Sn(s)-0.14Ni"(aq) + 2 e NI(s)-0.25Co2 (aq) + 2 e- Co(s)-0.28Ca*(aq) + 2 e-Cd(s)-0.403Cr"(aq) + e Cr²*(aq)-0.41Fe"(aq) + 2 e Fe(s)-0.44

Answered: How many grams of nickel metal will be…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 70QRT

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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)?
In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?
Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is 2Cl(aq)Cl2(g)+2e How long will it take to produce 2.00 kg of chlorine if the current is 5.00 102 A?
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)?
Using values from the table of standard reduction potentials, calculate the cell potentials of the following cells. (a) Fe(s)|Fe2+(aq)Hg2+(aq)|Hg(l) (b) Pt(s)|Fe2+(aq),Fe3+(aq)MnO4(aq),H+(aq),Mn2+(aq)|Pt(s) (c) Pt(s)|Cl2(g)|Cl-(aq)Au+(aq)|Au(s)
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
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?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
A current is passed through a solution of copper(II) sulfate long enough to deposit 14.5 g of copper. What volume of oxygen is also produced if the gas is measured at 24 °C and 0.958 atm of pressure?

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How many grams of nickel metal will be deposited from a solution that contains Ni²* ions if a current of 0.704 A is applied for 67.7 minutes. grams