X(s)|X4+ (0.87 M) || Mn O4 1 minus (1.61 M)|Mn2+ (2.98 M)|H+ (1.49 M) The reduction potential for X4+ is 2.22 V. The reduction potential for Mn O4 1 minus is 1.51 V What is the potential of this non standard cell (in Volts)?   options: -.70 V .22 V -.82 V

Consider the following standard reduction potentials. O₂(g) + 2H₂O(1) +4 Ca²+ (aq) +2e - 40H (aq) E° = 0.401 V Ca(s) E= -2.868 V E°

Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [A13+] to have changed by 0.46 mol/L. (Assume T= 25°C.) V Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors Supplemental Data

True or False: The reaction, S₂082- + Ni(OH)2 + 2OH2SO42- + NiO2 + 2H₂O, will occur spontaneously under standard state conditions. Following are the standard reduction potentials that may be useful: NiO2 + 2H₂O +2e=Ni(OH)2 +2OH E = 0.49 V S2082 +2e=2SO4²- True False E° = 2.01 V

If the potential for the following electrochemical cell is determined to be -0.525V SCE || Ag(CN)2 (7.5x10³M), CN (0.025 M) | Ag ESCE = 0.244V, E° Ag+/Ag = 0.799V, Calculate Kf for the reaction Ag* + 2CN¯ ± Ag(CN)2

156. Subject  :- Chemistry

A.  From the reaction as shown below, calculate the Standard Cell Potential of a Galvanic Cell that uses the half-reactions shown below.                              Cr3+    +    3e-    ------->     Cr               Eo = -0.73 V                             Al3+    +    3e-    ------->     Al              Eo = -1.66 V B. A galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V at 50oC. What is the concentration of CuSO4 in the cathode compartment?         Zn(s)   +   Cu(aq)2+   ------->   Zn(aq)2+   +   Cu(s)          Eo = 1.10 V Use:E = Eo - (RT/nF) + lnQ