Consider a galvanic cell based on the following line notation at 299 K: Cr|Cr 3+

Question

Consider a galvanic cell based on the following line notation at 299 K:

Cr|Cr3+||Cd2+|Cd

where the standard cell potential is 0.33 V. What will the following changes do to the potential of the cell?

increase potential decrease potential no change in potential  Add water to the anode portion of the cell
increase potential decrease potential no change in potential  Decrease the mass of the Cd
increase potential decrease potential no change in potential  Add equal amounts of water to both the anode and cathode portions of the cell

Explanation / Answer

the reaction taking place is:

Cr (s) + Cd2+ (aq)   —> Cr3+ (aq) + Cd (s)

formula for calculating E cell is

E = Eo - (0.0592/n) log {[Cr3+]^1/[Cd2+]^1}

Add water to the anode portion of the cell

This means adding water to Cr cell

This will decrease the concentration of Cr3+

So, E will increase as per above equation

Answer: increase

Decrease the mass of the Cd

mass do not appear in the equation of E

So, mass will not effect E

Answer: No change

Add equal amounts of water to both the anode and cathode portions of the cell

We are changing the concentration of both by same amount

So, E will not change

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.