Quiz - Electrochemistry

Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s)

• E_CELL=E⁰_CELL-0.0591/6 log[Mg2+]³/[Al3+]²

• E_CELL=E⁰_CELL-0.0591/6 log[Al3+]²/[Mg2+]³

• E_CELL=E⁰_CELL+0.0591/3 log[Mg2+]³/[Al3+]²

• E_CELL=E⁰_CELL-0.0591/3 log[Mg2+] /[Al3+]

Given the standard reduction potentials, E^o of iron is -0.44V and E^o of oxygen is 1.23V.

what will be the emf of the cell?

• -0.79V

• -1.67V

• 1.67V

• 0.79V

At equilibrium

• Cell potential will be zero

• Equilibrium constant becomes equal to electrode potential

• Equilibrium constant becomes zero

• Cell potential becomes unity

For this electrochemical cell, what is the expected observation at cathode?

• Copper metal dissolves

• reddish brown solid deposited

• Silvery grey solid deposited

• Silver metal dissolves

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu²⁺/Cu = 0.34V

Zn²⁺/Zn = -0.76V

• Cu

• Zn

• CuSO4

• ZnSO4

Which metal is the negative electrode?

• zinc

• copper

What would be the theoretical cell potential of the previous electrochemical cell?

• 1.05V

• -1.05V

• 0.55V

• -0.55V

What is the Nernst equation used for in electrochemistry?

• Calculating the pH of a solution

• Determining the cell potential under non-standard conditions

• Measuring the temperature of a reaction

• Finding the concentration of a solute

Which of the following is a component of the Nernst equation?

• Faraday's constant

• Planck's constant

• Avogadro's number

• Boltzmann's constant

• The change in free energy

• The temperature dependence of the cell potential

• The standard cell potential

• The equilibrium constant