E°cell = E red - Eoxi
= 0.339 - (-0.440) = 0.779 V
Ecell = E°cell - 0.059/n . Log oxi/red
= 0.779 - 0.059/2 . Log 0.0044/0.14
= 0.8233 V
Also reaction is spontaneous as Ecell value is positive
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2+ (0.15 M) Fe2+ (0.0039 M) Fe(s) E =-0.440 V E+Cu = 0.339 V Fe2+/Fe Is the electrochemical cell spontaneous or not spontaneous -0.779 Ecell = as written at 25 C? not spontaneous spontaneous о Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 'C Pt(s) Sn2 (0.0024 M), Sn4+ (0.12 M) |...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2 (0.12 M |Fe2 (0.0012 M) Fe(s) E2 =-0.440 V Efe/Fe = 0.339 V Cu2t/Cu Is the electrochemical cell spontaneous or not spontaneous Ecell V as written at 25 °C? not spontaneous spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2(0.0060 M), Sn4+(0.14 M) Fe3+(0.13 M), Fe2+(0.0056 M) Pt(s)...
Answers and detailed explanations For the following electrochemical cell, calculate the potential and determine if the cell reaction is spontaneous as written at 25 °C. Cu(s)|Cu2+(0.15 M)||Fe2+(0.0020 M)|Fe(s) Ecuaticu = 0.339 V Efez-ffe = -0.440 V Ecell = Determine if the cell reaction is spontaneous as written. O spontaneous O not spontaneous
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 ∘ C . Cu ( s ) ∣ ∣ Cu 2 + ( 0.13 M ) ∥ ∥ Fe 2 + ( 0.0011 M ) ∣ ∣ Fe ( s ) E ∘ Cu 2 + / Cu = 0.339 V E ∘ Fe 2 + / Fe = − 0.440 V E cell = V
4. Use the table below to provide a redox reaction involving the spontaneous oxidation of Cr (balance your final reaction and provide the Ecell). Half-reaction E (V) Cr3+ (aq) + 3e Cr(s) -0.74 Fe(s) -0.440 Fe3+ (aq) + → Fe2+ (s) +0.771 Sn4+ (aq) + 2e Sn2+ (aq) +0.154 Fe2+ (aq) + 2e-
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 1.05x10-4 atm, the CT concentration is 1.19M, and the Fe2+ concentration is 1.17M ? Cl2(g) + Fe(s) >2CI+ (aq) + Fe2+(aq) Answer: v The cell reaction as written above is spontaneous for the concentrations given V - true false Submit Answer Retry Entire Group 9 more group attempts remaining atm, the H* concentration is What is...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
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...
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe(s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn(aq) +2Cr(s) →2Cr" (aq) +35n²+ (aq)
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.08 atm, the F- concentration is 3.49×10-3M, and the Fe2+ concentration is 4.58×10-4M ? F2(g) + Fe(s)2F-(aq) + Fe2+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given: _____ (true/false)
> You have the red and oxi the wrong way round. E0cell=-0.779V, not 0.779V
Quinten Maas Mon, Jan 17, 2022 4:55 AM