Use the Nernst equation to calculate [Ag+] when [Cu2+] = 0.012M and ΔEcell= 0.410 V.
Use the Nernst equation to calculate [Ag+] when [Cu2+] = 0.012M and ΔEcell= 0.410 V.
Use the table of Standdard Reduction Potentials and the Nernst Equation to calculate the concentration of Cu2+ present in the Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled with a) Zn/Zn2+ b) Ag/Ag+ Table 2 has your measured voltages for these cells. SHOW YOUR SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE CALCULATED [Cu2+] CONCENTRATION. Table 2: METAL Mg Ag Ni Zn Pb Cu 1.230 V 0.642 V 0.030 V 0.648 V 0.256...
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
Part C. Effect of Concentration on Cell Potentials • Ecall for the Cu(s). Cu2+||Ag*, Ag(s) system: 0.450 V 0,851 v • Ecate for the Cu(s). Cu2+||Ag, Ag(s) system after the addition of 6M NH: • Write the balanced redox reaction for the entire cell: • • How many electrons are transferred? Use the Nernst Equation (given below) to calculate the concentration of Cu left in the solution Een = Ecen (0:0257) in (1960 [Cu2+] =
Use the Nernst equation to calculate Ecell for each of the following cells. Ag(s)|Ag+( 0.34 M )||Cl−( 0.095 M )|Cl2(g, 0.50 bar )|Pt(s) Thank you for any help
When doing a Nernst equation, how do you calculate n? I know for something like Zn|Zn2+(1.0 M)||Cu2+(1.0 M)|Cu where you have 2+ and 2+ n would be 2, but what about something like Pb|Pb2+(1.0 M)||Ag+(0.10 M)|Ag where you have 2+ and + I'm confused and can't find an answer anywhere
Compare the potentials between the Ag/Ag+ and Cu/Cu2+ half cells before and after adding excess NH3 to the Cu/Cu2+ half cell. Did the potential increase or decrease? Explain the result in terms of the Nernst equation.
C152-02 Class Practice Chapter 21 Practice 4 Calculate the reduction potential of the Cu2+/Cu electrode when Cu2+1 -1.0 x10 the table of standard reduction potentials and the Nernst Equation) M. (hint: use A cell is constructed by immersing a strip of silver in 0.10 M AgNO, solution and a strip of lead in 1.0 M Pb(NO3), solution. A wire and salt bridge complete the cell. What is the potential for the cell? Chint: use the Nernst Equation to determine the...
Choose the correct Nernst equation for the cell Zn + Cu2+ à Zn2+ + Cu E = E° - 0.0296 log(Cu / Zn) E=E° - 0.059 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log(Zn / Cu) E = E° - 0.0296 log([Zn2+] / [Cu2+]) E = E° - 0.0296 log([Cu2+] / [Zn2+]) 20 points
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value with th cell potential you measured. E = E* - 0.0592 / n * logQ **So I believe this is the equation that I would use. However, i'm don't know what E* is suppose to be...** The my electrochemistry experiment the cell potential that i measured were: 0.130V, 0.115V, and 0.110V (average cell potential = 0.118V) The concentration of the copper...
Class Practice C152-02 Chapter 21 Practice 4 Calculate the reduction potential of the Cu2/Cu electrode when [Cu] - 1.0 x108 M. (hint: use the table of standard reduction potentials and the Nernst Equation) A cell is constructed by immersing a strip of silver in 0.10 M AgNO, solution and a strip of lead in 1.0 M Pb(NO) solution. A wire and salt bridge complete the cell. What is the potential for the cell? (hint: use the Nernst Equation to determine...