Problem: Concentration cell based on the Ni2+-Ni cell reaction. (a) Concentrations of Ni2+(aq) in the two half-cells are unequal, and the cell generates an electrical current and a voltage. (b) The cell operates until [Ni2+] is the same in the two half-cells, at which point the cell has reached equilibrium and the emf goes to zero.Which electrode, if any, loses mass as the reaction proceeds?

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We’re being asked to determine which electrode loses mass as the reaction proceeds. We’re given the following diagram:

Recall that a voltaic or galvanic cell is an electrochemical cell that is spontaneous and produces electricity


Let's recall some parts of the galvanic cell:

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Problem Details

Two diagrams show two beakers, connected by a salt bridge and a wire.  The beaker on the left contains an Ni anode and the beaker on the right contains an Ni cathode. a) The left (anode) beaker contains a 1.00 times 10-3 molar Ni2+ concentration, and the right (cathode) beaker contains a 1.00 molar Ni2+ concentration. Electrons travel left to right through a wire from the Ni anode to the Ni cathode, producing 0.09 volts. b) After discharge, the Ni2+ concentration in both beakers is 0.5 molar and no voltage is produced.

Concentration cell based on the Ni2+-Ni cell reaction. (a) Concentrations of Ni2+(aq) in the two half-cells are unequal, and the cell generates an electrical current and a voltage. (b) The cell operates until [Ni2+] is the same in the two half-cells, at which point the cell has reached equilibrium and the emf goes to zero.

Which electrode, if any, loses mass as the reaction proceeds?

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What scientific concept do you need to know in order to solve this problem?

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