Question

You are given an electrochemical cell where the chemical reaction involves a silver complex. A silver metal bar is used as the positive electrode. The electrochemical potential for this cell is given by: E = EºAg+/Ag - 0.0592 (volts) * log(1/[Ag+]) For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag. This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at equilibrium?

          You are given an electrochemical cell where the chemical reaction involves a silver complex. A silver metal bar is used as the positive electrode. The electrochemical potential for this cell is given by:
E = EºAg+/Ag - 0.0592 (volts) * log(1/[Ag+])

For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag.

This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at equilibrium?

Added by Michael R.

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