A battery is an example of a galvanic cell. Use the Nernst equation to explain why a battery dies.
4. Use the chemical equation for the redox reaction and the Nernst equation to explain the following: a. A battery using the cell "CdCd (1.5M)||Ni?(1.5M)Ni" would eventually die "its potential would get too low to power a device") even though neither the Cd nor the N? is completely gone. b. Would you expect a battery using the cell Zn|Zn2+||Fe Fe?*|Pt to last longer than the cell in part a?
O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell. A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Mno (ae)+ 16H (a)+SPb (G)2Mn2 (a)+8H,0 ()+SPo (a) Suppose the cell is prepared with 1.5s M MnO and1.53 MH in one half-cell and 0.623 M Mn2 and 259 M Pb2 in the other Calculate the cell voltage under these conditions. Round your answer to 3 significant digits
III O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr + (aq) +3Ca (s) -- 2Cr (s) +3Ca²+ (aq) 2+ Suppose the cell is prepared with 0.699 M Cr3+ in one half-cell and 6.35 M Ca? in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 미미 X ? Check
O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo, (aq)+4H (aqg) +Fe (s)2VO2 (ag)+2H20 ()+Fe2(ag) Suppose the cell is prepared with 4.61 M VO, and 1.11 MH in one half-cell and 7.93 MVO and 4.62 M Fein the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. II
Use the Nernst equation to calculate the concentration of the unknown solution. Base this on your experimental voltage of 0.4410 V for the galvanic cell with silver combined with your copper half-cell. Use the unrounded [Cu2+] value of 0.04969 M and the unrounded value of the constants. E(cell) = 0.462 V Ag+ + e- → Ag(s) E(knot)= 0.799V Cu2+ + 2e- → Cu(s) E(knot)=0.337V
Use the Nernst equation to derive an equation relating the voltage of the cell (E_cell) consisting of a glass electrode and a silver/silver chloride reference electrode, to the pH of a solution. Define all variables in the equation.
What is a reversible galvanic cell? Why is the Nemst equation insufficient to determine the emf of a Daniel cell?
Use the Nernst equation to calculate the expected voltage of the concentration cell before the addition of the 10 extra drops of 0.10 M copper(II) nitrate solution. Use your experimental temperature. How did the addition of 10 drops of 0.10 M cupric nitrate affect the concentration cells voltage? Why? Temp. 21C E=91V 10 drops 75.8V
4. A practical galvanic cell is colloquially known as a "battery". Is Faraday's law in any way applicable to using a battery (hence a galvanic cell)? If so, how? (Hint: Did you see the waterfall or water + gravity analogy in the tutorial? Difference in height is not the only important waterfall parameter). 5. Ideally, determination of cell emf is a steady-state experiment with no net change in concentrations of ions and no current flowing. However, using a battery (galvanic...
3. Explain why the cell potential for an operating galvanic cell decreases over time but does not change from a positive value to a negative value. T A