Electrochemistry Mock Tests

The amount of electricity required to deposit 1 mole of aluminium from AlCl3 is:

In the conductometric titration of a strong acid (HCl) with a strong base (NaOH), the conductance curve typically shows:

The standard electrode potential (E°) for a cell reaction that is spontaneous must be:

The number of moles of electrons required to reduce 1 mole of Cr₂O₇²⁻ to Cr³⁺ is:

A galvanic cell is constructed as follows: Zn(s) | Zn²⁺(aq, 0.01 M) || Cu²⁺(aq, 1.0 M) | Cu(s) at 298 K. Given E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = −0.76 V, what is the cell potential under these non-standard conditions? (Use the Nernst equation with the approximation 2.303RT/F = 0.0591 V at 298 K.)

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)

A concentration cell is constructed with two silver electrodes immersed in solutions of Ag⁺ ions at different concentrations: Ag(s) | Ag⁺(0.001 M) || Ag⁺(0.1 M) | Ag(s) at 298 K. What is the cell potential E_cell? (For a concentration cell, E°_cell = 0 because both half-cells involve the same redox couple. The Nernst equation gives: E_cell = (RT/F) × ln([Ag⁺]_cathode/[Ag⁺]_anode), using the approximation 2.303RT/F = 0.0591 V at 298 K.)

What is the standard electrode potential (E°) of a cell if ΔG° for the cell reaction is negative?