APPENDIX 1: STANDARD REDUCTION POTENTIALS IN AQUEOUS SOLUTIONS NOTE: Higher Eo m
ID: 1039505 • Letter: A
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APPENDIX 1: STANDARD REDUCTION POTENTIALS IN AQUEOUS SOLUTIONS NOTE: Higher Eo means more easily reduced. HALF-REACTION Eo(V) 2.87 1.82 1.50 1.36 Co++e Co2 Cl2(g)+2e2CI 02(g) +4H4e2H200) Br2(1) + 2e-? 2Br 1.07 0.92 0.85 0.80 Hg". + 2e-? Hg(1) Ag eAg(s) 0.77 12(s) +2e ? 21. Cu eCu(s) Cu2+ +2e Cu(s) 0.52 0.34 0.15 0.15 0.14 S(s) +2H'+ 2eHS(g) 2H +2e H2(g) 0.00 -0.14 0.25 -0.28 -0.34 -0.40 -0.41 Sn2 +2e Sn(s) Ni2+ +2eNi(s) TI++ e-? T1(s) Cd2+ +2e-? Cd(s) Cr3++ e-? Cr2+ Fe2+eFe(s) -0.74 0.76 Zn2. + 2e- Zn(s) ? Al+ +3eAl(S) Be2++ 2e-? Beis) Mg2++ 2e-? Mg(s) Na +e Na(s) Ca2 +2eCa(s) Sr2+ +2e-? Sr(s) Ba2+ + 2e--+ Bals) Rb++ e-? RD(S) 2.37 2.71 -2.87 -2.89 -2.90 -2.92 -2.92 -2.92 -3.05 Cs'+e Li++ e- Cs(s) ? Li(s)Explanation / Answer
The more positive the standard reduction potential of the cation, the more difficult it is to oxidize the metal .
the table explains which metal is a good reducing agent .
the reduction potential table tells us that metals copper, silver , gold are less reactive than hydrogen . since their reduction potential is more positive than hydrogen . It shows these metals are less reactive than hydrogen and they do not replace hydrogen from water or acid. similarily for metal-displacement reactions: Zinc can displace copper from copper sulphate solution but the reverse case is not possible .
therefore the activity of metal is related to the above table of appendix-I