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A copper electrode is immersed in a 0.1M solution of CuSO4 and a zinc electrode is immersed in 0.1M solution of ZnSO4. Both the solutions are connected with a salt bridge. If the standard reduction potentials of Cu2+/Cu and Zn2+/Zn are +0.34V and -0.76 V respectively, calculate the potential difference between the two electrodes at 25°C.

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To calculate the potential difference between the two electrodes, we can use the Nernst equation. However, since both solutions have the same concentration  0.1M , the Nernst equation simplifies to the difference in standard reduction potentials.The cell potential  E_cell  can be calculated using the following equation:E_cell = E_cathode - E_anodeIn this case, the copper electrode has a higher standard reduction potential, so it will act as the cathode, and the zinc electrode will act as the anode.E_cathode = +0.34 V  Cu2+/Cu E_anode = -0.76 V  Zn2+/Zn Now, we can calculate the cell potential:E_cell =  +0.34 V  -  -0.76 V E_cell = 0.34 V + 0.76 VE_cell = 1.10 VThe potential difference between the two electrodes at 25C is 1.10 V.

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