A cell given by the notation below has an initial potential 0.118 V. Calculate the value of x.
Pt, H2 (1 atm)| H+ (10‐6 M) || H+ (x M) | H2 (1 atm), Pt
Please look at the below image it will help you.
A cell given by the notation below has an initial potential 0.118 V. Calculate the value of x. Pt, H2 (1 atm)| H+ (10‐6...
For the cell shown, the measured cell potential, ?cell, is −0.3629 V at 25 °C. Pt(s) | H2(g,0.899 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g)?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)?o=−0.403 V Calculate the H+ concentration. [H+]=
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
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!
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
For the cell shown, the measured cell potential, Ecell, is -0.3711 V at 25 °C Pt(s) H2(g, 0.865 atm) | Ht (aq,? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H"(aq) + 2е — H2(g) Eo = 0.00 V Cd2+(aq)2 e - Cd(s) Eo =-0.403 V Calculate the Ht concentration М
please help! :(
Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq, 0.0010 M) || Fe3 + (aq 0.0010 M), Fe2 + (aq, 0.010 M) | Pt (s) a) Write the reaction formula for the cell b) Calculate the normal potential of the redox pair Fe3 Fe2+
The cell potential of this cell is observed to be
0.445v Calculate the pH for the H+/H2 half cell
please explain the use of the half reaction in terms of the signs,
positive and negative in the equations.
The cell potential of this electrochemical cell is observed to be 0.445 v. Calculate the pH in for the H+H2 half cell Zn (s)| Zn2+ (2.5 M) || H*(??)[H2 (g. 4.5 atm)|Pt(s)
Given the measured cell potential, Ecell, is-0.3583 V at 25 °C in the following cell, calculate the Ht concentration Pt (s)|H2lg, 0.795 atm)lH (aq, ? M)l|Cd2 (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 2H+(aq) + 2e- H2(g) E0.00 V E-0.403 V ? 2 + Number H0.21
If the potential of a Zn-H+ cell (see below) is 0.45 V at 25 C when the [Zn2+] = 1.0M and PH2 = 1 atm, what is the pH of the cathode solution? Zn(s)|Zn2+(aq)|| H+(aq)|H2 (g)|Pt
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.