___What is the standard electrode Standard Reduction Potentials E potential for
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___What is the standard electrode Standard Reduction Potentials E potential for a voltaic cell constructed in the appropriate way from these two half-cells?(A) -1.02 V (B) 046 V (C) 0.64 V (D) 1.02 V ____ Balance this ionic equation for a redox reaction, using only whole number coefficients. ?MnO_4^- (aq) + ? Fe^2+ (aq) + ?H_3O^+(aq) rightarrow ?Mn^2+ (aq) + ?Fe^3+(aq) + ?H_2O What is the coefficient for Fe^2+ in the balanced equation? (A) 1 (B) 3 (C) 4 (D) 5 ____In this reaction, which substance behaves as the oxidizing agent? Pb() + PbO_2 + 2H_2SO_4 (aq) rightarrow 2PbSO_4 + 2H_2O (A) Pb (B) PbSO_4 (C) PbO_2 (D) H_2SO_4 ____which change requires an oxidizing agent to produce the indicated product? (A) S_2O_3^2- rightarrow S_4O_4^2- (B) Zn^2+ rightarrow Zn (C) O ClO^- rightarrow Cl^- (D) SO_3 rightarrow SO_4^2- Which statement is true for this reaction? Fe(s) + Cu^2+(aq) rightarrow Cu(s) + Fe^2+(aq) (A) Cu^2+ is oxidized. (B) Cu^2+ gains in oxidation number. (C) Cu^2+ is reduced. (D) Fe is reduced.Explanation / Answer
31)
from data table:
Eo(Cr3+/Cr(s)) = -0.74 V
Eo(Co2+/Co(s)) = -0.28 V
the electrode with the greater Eo value will be reduced and it will be cathode
here:
cathode is (Co2+/Co(s))
anode is (Cr3+/Cr(s))
The chemical reaction taking place is
Co2+ + Cr(s) --> Co(s) + Cr3+
Eocell = Eocathode - Eoanode
= (-0.28) - (-0.74)
= 0.46 V
Answer: B
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