Q. 33.5( 2 Votes )
E° values of some redox couples are given below. On the basis of these values choose the correct option.
E° values: Br2/Br- = 1.09; Ag+ / Ag(s) = 0.80
Cu2+ /Cu(s) = + 0.34; I2(s) /I = + 0.54
A. Cu will reduce Br-
B. Cu will reduce Ag
C. Cu will reduce I-
D. Cu will reduce Br2
Answer :
Reducing agents should have the ability to undergo oxidation that implies the property to easily loose electrons. Consequently the coupling element should have a greater tendency to attract the donated electron. As I- and Br- already are reduced ions so they cannot further undergo reduction. Between Ag and Br we can find from electrochemical series that the reduction potential of Br2 is more as compared to Ag.
Thus Cu will reduce Br2 as follows:
Corresponding [potential for the developed cell is
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PREVIOUSThe more positive the value of EV, the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.E° Values: F3+/Fe2+ = 0.77; I2 (s) /I = +0.54;Cu2+ /Cu = + 0.34; Ag+ /Ag = + 0.80VNEXTUsing the standard electrode potential, find out the pair between which redox reaction is not feasible.E°Values: Fe3+/ fe2+ = +0.77; I2/I- = +0.54;Cu2+/ Cu = -0.34; Ag+ /Ag = + 0.80 V
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Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible:
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NCERT - Chemistry Part-II