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
Use the Nernst equation to calculate Ecell for each of the following cells. Ag(s)|Ag+( 0.34 M...
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell° for this galvanic cell? If a more complete description of the cell is Ag(s)│Ag(NO3)(aq, 0.50 M)││KMnO4(aq, 0.50 M), HCl(aq, 2.5 M), Mn(Cl)2(aq, 0.01 M)│Pt(s), Ag(s) what is Ecell? What is the balanced, spontaneous cell reaction for the cell conditions given in b.?
Question9 Write the Nernst equation of the following cells at 298 K: (i) Mg(s) | Mg210.001 M) Il Cu2+(0.0001 M) I Cu(s) (ii) F e(s) l Fe,"(0.001 M) İl H+(1 M)1Hz(g)( l bar) I Pt(s) (İİİ) Sn(s) | Sn2+(0.050 M) Il H+(0.020 M) I H2(g) (1 bar) | Pt(s) (iv) Pt(s) | Br(ol Br-(0.010 M) Il H'(0.030 M) I H2(g) ( l bar) I Pt(s). Question 10 In the button cells widely used in watches and other devices the following...
Use the Nernst equation to calculate the corresponding voltage if the Cl (9) were at 4.0 atm, the Zn2+ were 0.01 M, and the Cl- remains at 1 M for the reaction Zn(s) + Cl, (g) Zn- (aq) + 2 C1(aq) E° = 2.122 V
Use the Nernst equation to calculate [Ag+] when [Cu2+] = 0.012M and ΔEcell= 0.410 V.
7. The following system has Ecell = 0.8401 V at 1000 K: (10 pts) Ag(s) + 12 Cl2(g) → AgCl(1) If the ang = a Agci = 1 and acı2 = 0.76, calculate the values of the Ecell and the equilibrium constant, K.
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
I just want to double check my work for Q1, 2, 3 in the blank
spaces and the Nernst equations.
Concentration Cells 1) Concentration cell #1 : Which solution is being reduced, the IM Cu2 or the 0.001M Cu? VE 90 What was the measured cell potential for the 1M Cu/0.001 M Cu concentration cell? 14,S mV Measured Ecel= Use the Nernst equation to calculate the expected cell potential for the 1M Cu/0.001M Cu concentration cell; refer to the experimental...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
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...
For which of the following voltaic cells will Ecell be greater than Eºcell? Pb(s) | Pb2+(0.0200 M) || Ag+(0.0200 M)| Ag(s) Pb(s) | Pb2+(0.00200 M) || Ag+(0.200 M)| Ag(s) Pb(s) | Pb2+(0.200 M) || Ag+(0.200 M)| Ag(s) Pb(s) | Pb2+(0.00200 M) || Ag+(0.0200 M)| Ag(s) Pb(s) | Pb2+(0.200 M) || Ag+(0.0200 M)| Ag(s)