. B will reduce X. e. Y will reduce A Which of the following metals can be oxidi
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. B will reduce X. e. Y will reduce A Which of the following metals can be oxidized by H'under standard conditions? Show your arguments. Cu, Zn, Ag, Sn Ag(a?)+e-Ag(s) Cu(aq) +2e Cu(s) Cu(aq)+e Cu'lag) Snt (ag)+ 2e-Sn(a) Sn(ag) +2e-Sn(s) Zn2 (ag)+ 2e-Zn(s) E -0.80 V E 0.34 V 0.15 V E 0.13 V E"--014 V Answer: for the reaction of oxidation of the metal by H+ to be spontaneous, the cell made from SHE as cathode (H+ is itself reduced) and the metal as anode should have a positive cell potential. E.By doing the calculations for each of the given half cells, we find that only the selected two metals fulfill the requirementExplanation / Answer
2H+ + 2e- -----> H2 ; E0 = 0
Sn+2(aq) + 2e- -----> Sn(s) ; E0 = -0.14V
Zn+2(aq) + 2e- -----> Zn(s) ; E0 = -0.76V
Reduction potetial of Sn and Zn are less than compare to H. So both the metals undergo oxidation with H+ ions.
Hence the cell reaction is,
Sn(s) + 2H+(aq) ------> H2(g) + Sn+2(aq) ; E0 cell = 0 - (-0.14) = 0.14 V
Zn(s) + 2H+(aq) ------> H2(g) + Zn+2(aq) ; E0 cell = 0 - (-0.76) = 0.76 V
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