Pretest5.5

Nernst equation for

Mg(s) | Mg²⁺(0.001M) || Al³⁺(0.001 M) | Al(s)

• E_Cell=E⁰_Cell − 0.0592/6 log [Mg²⁺]³/ [Al³⁺]²

• E_Cell=E⁰_Cell +0.0591/3 log[Mg²⁺]³/[Al³⁺]²

• E_Cell=E⁰_Cell − 0.0592/6 log [Al³⁺]²/ [Mg²⁺]²

• E_Cell=E⁰_Cell −0.0591/3 log[Mg²⁺] /[Al³⁺]

How to increase cell potential, E_cell based on this Nernst equation:

• Increase temperature

• Decrease concentration Ni²⁺

• Increase concentration Ni²⁺

• Choose E^ocell anode and cathode the positive value

Caculate the E_cell for the following galvanic cell.

Zn(s)|Zn²⁺ (aq, 1.0M) || Ag⁺ (aq,1.5M)|Ag(s)

• 0.32 V

• 0.33 V

• 1.84 V

• 1.85 V

Calculate the cell potential, E_cell of the electrochemical cell in with reaction

Pb²⁺ + Cd → Pb + Cd²⁺ .

Given that E^o_cell = 0.277 V,

[Cd²⁺] = 0.02M, and [Pb²⁺] = 0.2M.

• 0.207 V

• 0.307 V

• 0.255 V

• 0.355 V