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.
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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...
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...
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:...
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...
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...
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...
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...
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...
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
Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V Use...
Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) E° = 1.10 V Use the Nernst equation to calculate the cell potential for the cell described with standard line notation below. Zn|Zn2+(0.5038 M)||Cu2+(0.3981 M)|Cu Units are not required. Report answer to three decimal places.
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value...
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...
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...
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+] =
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...
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