A concentration cell is constructed using two metal (M) electrodes with M2+ concentrations of  xM (cathode) and 10-5M (anode) in the two half-cells (x is larger than 10-5M so [M2+] of the anode is 10-5M). The cell potential at 25°C is 0.118 V. Determine the cathode concentration ([M2+ ]cathode). a. 3M b. 1M c. 0.1M d. 0.01M e. 0.5M

Consider the same diagram of a galvanic cell as in previous question,                        where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows:              Ag+(aq)   +  e–   -->  Ag(s);    Eo =   0.80 V             Ni2+(aq)  +  2e–  -->  Ni(s);     Eo = – 0.23 V          What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M.            (A) 1.15 V          (B) 1.30 V          (C) 0.76 V          (D) 0.91 V

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Consider an electrochemical cell made up of Cul Cu²+ and Ag Ag* half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 0-0 E = V X 00 Calculate the standard emf of a cell that uses the Cu Cu²+ and Ag|Ag half-cell reaction at 25 °C. Round your answer to 3 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. X 3