Consider the concentration cell constructed with two silver electrodes in 0.1M a

Question

Consider the concentration cell constructed with two silver electrodes in 0.1M and 1.0M silver nitrate solutions. Will electrons flow in this cell? if so , in what direction? Label the anode and the cathode. Write the half-reactions occuring at the anode and the cathode. If the current flows will it ever stop? when?

Cant post image, but the picture consists of 2 beakers, both with a Ag metal strip and a salt bridge. One beaker has 0.1M Ag+ and 0.1M No3- while the other beaker has 1M Ag+ and 1M NO3-

Explanation / Answer

Since the concentration of the ions is more in the higher concentration part so the no. of ions would ultimately result in the excess of electrons

which would result in the flow of ion in the reverse direction of the flow of electrons

so the current will flow from the 0.1 M container to the 1M container

and yes the current will stop when the concentration of ions in both the beakers will become equal ...

2 NO3-1(aq) + 4 H+1(aq) + 2e-1 ---------> 2 NO2(g) + 2H2O(l)
Ag+1(aq) + e-1 ---------> Ag(s)

so the two half cell reactions are given
and now we can find the Cell potential by the formula




E cell = E*cell- RT/nF ln [con of product ions/conc of reactant ions ]

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