A concentration cell Is constructed by placing identical Cu electrodes in two Cu

Question

A concentration cell Is constructed by placing identical Cu electrodes in two Cu2+ solutions. If the concentrations of the two Cu2+ solutions are 1.0 M and 0.002 M, calculate the potential of the cell. 0.080 V 1.2 V 0.030 V 1.0 V 0.020 V In voltaic cells, the salt bridge. is not necessary in order for the cell to work allows charge balance to be maintained in the cell acts as a mechanism to allow mechanical mixing of the solutions is tightly plugged with firm agar gel through which ions cannot pass drives free electrons from one half-cell to the other In the following voltaic cell: the electrodes arc connected by means of a membrane Zn/Zn^2+ is the cathode Zn/Zn^2+ is the anode the electrodes are connected by means of a membrane none of the above How many electrons flow in the following battery: 3e^- 2e^- 5e^- 6e^- zero Calculate delta epsilon for the following voltaic cell: Au Knowing that delta epsilon degree = +2.00V -0.5 V 2.00 V 1.94 V 7 V

Explanation / Answer

16) Cu2+ + 2e- ----> Cu

Number of electrons transferred = n = 2

Cell potential , Eo = -(0.059 /n) x log ([Cu2+]0.002 M / [Cu2+]1M)

= -(0.059/2) x log (0.002/1)

= +0.080 V

So option (A) is correct

17) (B) is correct

18) Zn/Zn2+(aq) // Cu2+(aq) /Cu

anode cathode

At anode oxidation takes place

At cathode reduction takes place

So option (C) is correct

19) option (D) is correct

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