Calculate the cell potential for the following cell at 25 ° C
Cd (s) | Cd (NO3) 2 (aq, 0.010 M) || KBr (aq, 0.050 M), Ag + (aq) | AgBr (s) | Ag (s)
using normal potentials E⦵ (Cd 2+ / Cd) = -0.40 V and E⦵ (Ag + / Ag) = 0.80 V, and the solubility of AgBr, which is 7.7 · 10-13.
Calculate the cell potential for the following cell at 25 ° C Cd (s) | Cd...
Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
Calculate the electrostatic potential of the cell at below 25 ° C .Pt (p) | H 2 (g, 200 kPa) | HNO 3 (aq, 0.10 M) || AgNO3 (aq, 0.0100 M) | Ag (s) E ° for Ag + + e- ® Ag (s) is 0.80 V.
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) II Ag+(aq, 0.55 M)1 Ag(s) Sn2+ (aq) + 2 e Ag+ (aq) + e- Sn(s) Ag(s) E = -0.14 V E = 0.80 V -0.84 V +0.86 V 0 -0.93 V +1.12 V O 0.92 V
Please answer BOTH parts to this question. Thanks (1) The equilibrium constant of the reaction 2 C3H6(g) C2H4(g) + C4H8(g) is found to fit the expression In K= A + B/T + C/T2 between 300 K and 600 K, with A = -1.04, B = -1088 K, and C = 1.51 10% K2. Calculate the standard reaction enthalpy at 400 K. (2) Consider the electrochemical cell Ag|AgBr(s)|KBr(aq,0.050 molal)||Cd(NO3)2 (aq,0.010 molal)|Cd. Calculate the cell potential.
16.2 cell potential for the following cell was measured to 0.889 V at 25 ° C. Pt (p) | H 2 (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 +.
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 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, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 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, Eº, are 2 H+ (aq) + 2e H (9) E' = 0.00 V Cd2+ (aq) + 2e - Cd(s) E' = -0.403 V Calculate the H concentration. [HT] = M