If your base metal is Nickel, which among the following metals can act as a sacrificial anode for it? EMF series metal Vo metal Au +1.420 V Cu +0.340 Pb - 0.126 Sn - 0.136 Ni - 0.250 Co - 0.277 Cd - 0.403 Fe - 0.440 - 0.744 - 0.763 Cr Zn Al - 1.662 - 2.363 - 2.714 Mg Na K - 2.924 A Tin (B) Lead Magnesium (D Copper

If your base metal is Nickel, which among the following metals can act as a sacrificial anode for it? EMF series metal Vo metal Au +1.420 V Cu +0.340 Pb - 0.126 Sn - 0.136 Ni - 0.250 Co - 0.277 Cd - 0.403 Fe - 0.440 - 0.744 - 0.763 Cr Zn Al - 1.662 - 2.363 - 2.714 Mg Na K - 2.924 A Tin (B) Lead Magnesium (D Copper

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

11. Consider the following reaction and its AG-AG• at 25.00 °C. 12 Coeside 2Ag*(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG =-88660 J/mol a. Calculate the standard cell potential, Ecellº, for the reaction. b. Calculate the equilibrium constant, K, for the reaction. Wtoxided what is reduced? CLEAREY
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V
The free energy change for the following reaction at 25 °C, when [Cd2*] = 1.17 M and [Cr+] = 8.47x10-3 M, is -207 kJ: 3ca**(1.17 M) + 2Cr(s)3Cd(s) + 2Cr³+(8.47x103 M) AG = -207 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Calculate AG° and K for the following reactions. Ag(S2O3)2* + Fe(CN)6* + Ag(s) + 2S20;? + Fe(CN)6*
Calculate AG for the following reaction. 2 Cr(s) +3 Cl2(aq) 2 Cr*t (ag) + 6 CI (aq) Hall-Reaction Hall-Reaction 5+ 20 2F Ag +e Ag Co +eCo HO, + 2H+ 2e 2H0 Ce+eCe PO, - 4H + So,+ 2 PhSO, + 2H,0 MaO,+ 4H + 3MaO, + 2H,0 2+ 2H + 10; 10," + HO Ma0,+ KH" + SeMa" + 4H,0 As +3 A PhO, + 4H + 2e + 2H,0 C+ 2e 20 Cr0,+ 14H" + de2Cr" + 7H0 0, + 4H + → 2H,0 MaOy + 4H +2 Ma+ 2H,0 10, + 6H + Se 4 + 3H,0 Be+ 2-2B vo," + 2H +e VO + H0 AuC+ 3 Au + 40 NO,+41 + 3eNO + 2H,0 2.87 0, + 2H0 + 4 4OH" Cu+ 2 Cu Hg C, + 22Hg + 20 Aa +e Ag +a So+ 4H + 2I1S0, + HO 0.40 0.34 027 022 0.20 1.99 182 1.78 1.70 016 1,68 160 151 2H + 20-H Fe + Fe P+ 2- 0.00 -0.006 -0.13 150 Sa+ 2e Sn -Q14 N4 2e- N PASO, + 2P+ So, C + 2e" Cd C" +eC 1.46 -035 -040 1.36 1.33 1.23 -041 1.21 1.20 -0.44 -G73 Za + 2 Za 2H,0 + 2e H, + 201 Ma"+ 2e Ma 1.09 100 -LI 0.99 0.96 0.954 0.91 0.80 A+3e Al -16 -223 -237 2Hg" + 2eHs" Ag +eAg H+2e2Hg H + 2e 2H Mg + 2eMg La+3 La Na" te-Na Ca+ 2eCa Ba+ 2Ba K* +eK -237 -271 -276 -290 -292 0, + 2H" + 2e-HO, MaO,+…