Consider a galvanic cell based on the following line notation at standard conditions and 298K: Sn...

Consider a galvanic cell based on the following line notation at standard conditions and 298K:

Sn | Sn²⁺ || Fe³⁺ | Fe

Which of the following changes WILL NOT change the potential of the cell?
Add equal amounts of water to each half cell
Replace the Fe electrode with a Pt electrode
Increase the concentration of Sn²⁺
Decrease the concentration of Fe³⁺
Replace the Sn electrode with a Pt electrod

Expert Solution

Addition of equal amounts of water to each half cell will not change the potential of the cell.

Explanation:

Option 2. The replacement of Fe-electrode with Pt-electrode will increase the standard potential (E^o) value of the cell. As a result, the potential of the cell changes.

Option 3. If you increase the concentration of Sn²⁺, the cell potential changes according to Nernst law.

The balanced cell reaction: 3Sn(s) + 2Fe³⁺(aq) 2Fe(s) + 3Sn²⁺(aq)

i.e. E_cell = E^o_cell - Log([Sn²⁺]³/[Fe³⁺]²)

Option 4. If you decrease the concentration of Fe³⁺, the cell potential changes according to Nernst law, mentioned above.

Option 5. The replacement of Sn electrode with a Pt-electrode will decrease the standard potential (E^o) value of the cell. As a result, the potential of the cell changes.

Option 1. If you add an equal amount of water to each half-cell, then the concentrations of Sn²⁺ or Fe³⁺ will not change. As a result, the cell potential will not change.

Amanda K answered 2 years ago

Consider a galvanic cell based on the following line notation at 295 K: Fe|Fe3+||Cu2+|Cu where the...

Consider a galvanic cell based on the following line notation at 295 K: Fe|Fe3+||Cu2+|Cu where the standard cell potential is 0.38 V. What will the following changes do to the potential of the cell? a) Add water to the anode portion of the cell increase potential decrease potential no change in potential b) Add equal amounts of water to both the anode and cathode portions of the cell increase potential decrease potential no change in potential c) Increase the mass...

Consider a cell based on the following line notation at 298 K: Cu | Cu2+ (0.237...

Consider a cell based on the following line notation at 298 K: Cu | Cu2+ (0.237 M) || Ni2+ (1.29 M) | Ni Given: Cu2+ + 2 e- → Cu Eo = 0.34 V Ni2+ + 2 e- → Ni Eo = -0.23 V How many of the following responses are true? 1. Decreasing the concentration of the Cu2+ will increase the concentration of the reaction 2. Using a Pt electrode in place of the Cu electrode will not change the potential...

consider a galvanic cell that is set up under standard conditions and allowed to react. How...

consider a galvanic cell that is set up under standard conditions and allowed to react. How many of the following responses are true? 1. Electrons are produced spontaneously at the anode electrode 2. Electrons will flow from the cathode half cell to the anode half cell 3. The mass of the cathode electrode will increase as the galvanic cell approaches being "dead" 4. The salt bridge acts as a second pathway for electrons to flow thereby "completing" the electrical circuit...

Given the following pair of half-reactions, fill in the line notation for a standard cell using...

Given the following pair of half-reactions, fill in the line notation for a standard cell using these two half-reactions. Since it is a standard cell, all concentrations will be 1 M, so do not enter concentrations. You have solid platinum (Pt) electrodes to use, where necessary. Do not include the physical state of the components, i.e., solid platinum would just be Pt. For subscript and superscripts use the model: Ag+ would be Ag^+ and SO42- would be entered as SO4^2-,...

Consider a galvanic cell based upon the following half reactions: Ag+ + e- → Ag;...

Consider a galvanic cell based upon the following half reactions: Ag+ + e- → Ag; 0.80 V Cu2+ + 2 e- → Cu; 0.34 V Which of the following changes will decrease the potential of the cell? Adding Cu2+ ions to the copper half reaction (assuming no volume change). Adding equal amounts of water to both half reactions. Adding Ag+ ions to the silver half reaction (assume no volume change) Removing Cu2+ ions from solution by precipitating them out...

Consider a galvanic cell based on the following half reactions: E° (V) Al3+ + 3e- →...

Consider a galvanic cell based on the following half reactions: E° (V) Al3+ + 3e- → Al -1.66 Ni2+ + 2e- → Ni -0.23 If this cell is set up at 25°C with [Ni2+] = 1.00 × 10-3M and [Al3+] = 2.00 × 10-2M, the expected cell potential is what?

Consider a galvanic cell based in the reaction Fe2+ + Cr2O72- → Fe3+ + Cr3+ in...

Consider a galvanic cell based in the reaction Fe2+ + Cr2O72- → Fe3+ + Cr3+ in acidic solution. What is the coefficient of Fe3+in the balanced equation? Reference: Ref 18-2 Select one: a. 3 b. 4 c. none of these d. 6 e. 2

Consider a galvanic cell based upon the following half reactions: Cu2+ + 2e- → Cu 0.34...

Consider a galvanic cell based upon the following half reactions: Cu2+ + 2e- → Cu 0.34 V Fe3+ + 3e- → Fe -0.0036 V How many of the following responses are true? 1. Decreasing the concentration of Cu2+ (assuming no volume change) will decrease the potential of the cell 2. Increasing the concentration of Fe3+ (assuming no volume change) will increase the potential of the cell 3. Adding equal amounts of water to both half reaction vessels will increase the...

Consider a galvanic cell based on the following two half reactions at 298 K: SRP Fe3+...

Consider a galvanic cell based on the following two half reactions at 298 K: SRP Fe3+ + e-  Fe2+ 0.77 V Cu2+ + 2 e-  Cu 0.34 V How many of the following changes will increase the potential of the cell? Why? 1. Increasing the concentration of Fe+3 ions 2. Increasing the concentration of Cu2+ ions 3. Removing equal volumes of water in both half reactions through evaporation 4. Increasing the concentration of Fe2+ ions 5. Adding a...

Consider a galvanic cell based upon the following half reactions: Ag+ + e- → Ag 0.80...

Consider a galvanic cell based upon the following half reactions: Ag+ + e- → Ag 0.80 V Pb2+ + 2e- → Pb -0.13 V How would the following changes alter the potential of the cell? Adding Ag+ ions to the silver half reaction (assume no volume change) Adding Pb2+ ions to the lead half reaction (assuming no volume change). Removing Pb2+ ions from solution by precipitating them out of the lead half reaction (assume no volume change). Adding equal amounts...

Question