Electrochemistry Mock Tests

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)

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

For the cell Zn(s) | Zn²⁺(1.0 M) || Cu²⁺(0.1 M) | Cu(s), E°cell = 1.10 V. What is the cell potential at 298 K? (2.303RT/F = 0.0591 V)

The standard electrode potential of a cell is determined by:

A current of 2.0 A is passed through an aqueous solution of CuSO₄ for 965 seconds. The mass of copper deposited at the cathode is (Atomic mass of Cu = 63.5, F = 96500 C/mol):

For the cell reaction Zn + Cu²⁺ → Zn²⁺ + Cu, the standard cell potential is 1.10 V. If [Zn²⁺] = 0.01 M and [Cu²⁺] = 0.1 M, the cell potential at 298 K is (log 10 = 1):

Which of the following is the correct order of reduction potential (most positive to most negative)?

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)