Using the formula
For the cell
n = 2 (represents loss of 2 electrons)
substituting the values in the equation, we get
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answer is 84907J/mol. help me solve this Use the following Fe potential diagram to calculate AGº...
7.53 Given the following electrode potentials at 25°C, Fe3+ +e- = Fe2+ E' = 0.771 V Fe2+ + e = Fe(s) E = -0.440 V calculate the electrode potential for [Fe3+ + e = {Fe E; = ? for
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) |...
help me solve this correctly Calculate the value of E for the galvanic cell made from these two half reactions when MnO4) = 0.010 M. [H] =0.20 M, [Mn?] = 0.020 M, [Fe3+] = 0.75 M, [Fe2+] = 0.30 M. Ece - OTO nF 75 Q: 1.02m] 6.30m 5 (-010[0.1073747 (0.05 .000 4 MnO4 +8H+ +5e → Mn2+ + 4H20 E° = 1.51 V Fe3+ + + Fe2+ Ecelli Ecell - (8. (8./4.J/mol) (E° = 0.77 V Product S496485) Treactants...
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)...
Half-reaction Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e - Fe(s) Fe3+ (aq) - Fe2+ (5) Sn+ (aq) + 2e - Sn2(aq) E (V) -0.74 -0.440 +0.771 +0.154 1. Calculate the standard cell potential for the voltaic cell based on the reaction below, given the table above: 35nt(s) + 2Cr (s) - 2 C (s) + 3 Sn () ANSWER: 2. Calculate the standard cell potential for the voltaic cell based on the reaction below, Riven the table above 3Feb...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Cu(s) Cu2+(0.14 M) | Fe2+(0.0044 M) Fe(s) Ecu?+Icu = 0.339 V Efez lfe = -0.440 V Ecell = v Is the electrochemical cell spontaneous or not spontaneous as written at 25 °C? O not spontaneous O spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2+(0.0048 M), Snº+(0.11 M) || Fe3+(0.12...
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+ (aq) + 2 C1 (aq) Write a cell diagram for this reaction In this reaction, calculate Eºcell under standard conditions Calculate AGº from the cell potential B. C. D. Calculate K from the cell potential. E. Predict the value of Ecell for this reaction in if the concentration of is 0.150 M, is 0.100 M and the concentration of Cl- is 0.010 M. Fe2+...
Calculate the cell potential for the reaction as written at 25.00°C, given that [Zn2+] = 0.758 M and [Fe2+] = 0.0140 M. Use the standard reduction potentials in this table. Zn(s) + Fe2+ (aq) = Zn²+ (aq) + Fe(s) Zn2+(aq) + 2e- → Zn(s) -0.76 Fe2+(aq) + 2e- > Fe(s) -0.44
What is the expected standard cell potential for the following unbalanced reaction under basic conditions? MnO4-(aq) + Fe+2(aq) ⟶ Fe+3 (aq) + MnO2(s) Given: Fe3+ + e− ⟶ Fe2+ E1/2= 0.771 MnO4−+ 2 H2O + 3e− ⟶ MnO2 + 4OH− E1/2 = 0.558 A. -0.213 V B. +0.213 V C. -1.329 V D. +1.329 V E. None of the above