Electrochemistry

An electrochemical cell can behave like an electrolytic cell when

• E_cell = 0

• E_cell> E_ext 

• E_ext> E_cell 

• E_cell = E_ext

The quantity of charge required to obtain one mole of Aluminium from one mole of Al₂O₃ is

• 1F 

• 6F

• 3F

• 2F

The cell constant of a conductivity cell

• changes with change of electrolyte. 

• changes with change of concentration of electrolyte. 

• changes with temperature of electrolyte.

• remains constant for a cell. 

The positive value of the standard electrode potential of Cu²⁺/Cu  indicates that

• this redox couple is a stronger reducing agent than the H⁺/H₂ couple.

• this redox couple is a stronger oxidizing agent than the  H⁺/H₂ couple

• Cu can displace H⁺from dilute acid. 

• H⁺can displace Cu ²⁺from dilute acid.

Conductivity of an electrolytic solution depends on

• pressure

• concentration of electrolyte.

• power of AC source.

• distance between the electrodes

What will happen during the electrolysis of aqueous solution of CuSO₄ by using Platinum  electrodes?

• Copper will deposit at the cathode. 

• Copper will deposit at anode. 

• Oxygen will be released at cathode.

• Copper will dissolve at anode.

What will happen during the electrolysis of aqueous solution of CuSO₄ in the presence of Cu electrodes?

• Copper will deposit at the cathode. 

•   H ₂ will be released at anode. 

• Oxygen will be released at cathode. 

•  Copper will deposit at anode.

Molar conductivity of ionic solution depends on

• density of the solution

•   distance between electrodes. 

• concentration of electrolytes in solution. 

• surface area of electrodes.

For the given cell, Mg | Mg ²⁺|| Cu ²⁺|Cu

• Mg is cathode 

• Cu is anode 

• The cell reaction is Mg (s)+ Cu²⁺ (aq)→ Mg ²⁺   + Cu 

• Cu is the reducing agent 

The charge required for the reduction of 1 mol of MnO₄^-  to  MnO₂  is

•  1 F

• 3 F

• 5 F

• 6 F