Please show your work Given the following standard reduction potentials, Ag^+(aq) + e^- rightarrow Ag(s) E^degree...
Given the following standard reduction potentials Ag+(aq) + e- ↔ Ag(s) E = 0.80 V AgCN(s) + e- ↔ Ag(s) + CN-(aq) E = -0.01 V Calculate the solubility product of AgCN at 25°C. 4.3 &αχυτε; 10−14 2.3 &αχυτε; 1013 2.0 &αχυτε; 10−14 5.1 &αχυτε; 1013 None of the above
Given the following standard reduction potentials: H^+ (aq) + 2e^- rightarrow H_2(g) E degree = 0.00 V Fe^3+ (aq) + 2e^- rightarrow Fe(s) E degree = -0.43 V (a) What is the cell potential by combining the above two half-reactions to make a working voltaic cell (same as galvanic cell)? (b) Which species will be oxidized in anode? Write the half-reaction for the anode. (c) Write the overall reaction and balance the chemical equation for this working voltaic cell. (d)...
Given that E degree = 0.52 V for the reduction Cu^2+ (aq) + e^- rightarrow Cu(s), calculate E degree delta G degree, and K for the following reaction at 25 degree C: 2 Cu^+ (aq) rightwardsharpoonoverleftwardsharpoon Cu^2+ (aq) + Cu(s) E degree = V delta G degree = kJ K = times 10 Enter your answer in scientific notation.
What is Eº for the cell Mn| Mn2+ (aq) || Ag+ (aq) | Ag? Standard Reduction Potentials E° (V) Ag+(aq) + e + Ag(s) +0.80 Mn2+(aq) + 2e Mn(s) -1.18 V 1 2 3 Х 1
6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(aq)....
Calculate the E_cell^compositefunction for the following equation. Use these standard potentials Cu(s) + Ag^+(aq) rightarrow Cu^+(aq) + Ag(s) E_cell^compositefunction = Number _________ V
Step-by-Step approach please? Calculate the solubility product of silver iodide at 25 degree C given the following data: AgI(s) + e^- rightarrow Ag(s) + I^- I_2(s) + 2e^- rightarrow 2I^- Ag^+ e^- rightarrow Ag(s) A) 2.9 times 10^- 3 B) 1.9 times 10^- 4 C) 2.1 times 10^- 12 D) 9.0 times 10^- 17 E) 2.4 times 10^- 24 E degree (V) - 0.15 + 0.54 + 0.80
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+ (aq, 0.50 M)||I^- (aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e^- rightarrow Ag(s) + I^-(aq) E degree = -0.15 V Sn^4+ (aq) + 2 e^- rightarrow SN^2+ (aq) E degree= +0.15 V.
Consider the cell AgcAglo | Agen Ag(s) +0.80 V at which has the standard reduction potentials E°(anode) -0.15 V and E (cathode) 25°C. Calculate (a) the solubility constant of Agl and (b) its solubility at 25°C.
Question 7 (1 point) Saved Consider these metal ion/metal standard reduction potentials Cu2(aq)|Cu(s) Ag+1(aq)|Ag(s) Co2(aq)|Co(s) Zn+2(aq)]Zn(s) +0.34 +0.80 V -0.28 V -0.76 V Based on the data above, which one of the species below is the best oxidizing agent? 0 1 Cols) O2) Zn(s) 3) Cutlaq) 04) Culs) 5) Ag+h(aq)