Electrochemistry Mock Tests

The Nernst equation for the cell reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s) at 298 K is:

Which of the following is the correct order of reduction potential (decreasing order)?

The standard electrode potential for the cell Zn|Zn²⁺||Cu²⁺|Cu is (E°(Zn²⁺/Zn) = -0.76 V, E°(Cu²⁺/Cu) = +0.34 V):

In a Daniel cell (Zn|Zn²⁺||Cu²⁺|Cu), if the concentration of ZnSO₄ is increased tenfold while CuSO₄ concentration remains at 1 M, how does the cell EMF change? (E°cell = 1.10 V)

The number of electrons transferred in the reaction: Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O is:

During electrolysis of aqueous CuSO₄ using copper electrodes, the mass of copper deposited on the cathode is 6.35 g. The quantity of electricity required is: (Atomic mass of Cu = 63.5 g/mol, F = 96500 C/mol)

For the cell reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), E° = 1.10 V. If [Zn²⁺] = 0.1 M and [Cu²⁺] = 1.0 M at 298 K, what is the cell potential?

The same quantity of electricity that deposits 1.08 g of silver from AgNO₃ solution will deposit how much copper from CuSO₄ solution? (Atomic masses: Ag = 108, Cu = 63.5)