8) Does the following cell diagram represent at spontaneous process at 25°C? FeFe?' (0.15M)Cr(0.08M) Cr
For the following cell, at 25 ° C, Cr (s) | Cr (NO3) 3 (0.200 M) || Pb (NO3) 2 (0.060 M) | Pb (s) the cell potential was 0.589 V. Calculate the equilibrium constant for the following reaction at this temperature : 2Cr (s) + 3Pb2 + (aq) --- 2 Cr3 + (aq) + 3Pb (s)
6. Determine whether the following cell reaction is spontaneous or not at 25°C, and calculate a cell potential. Cu Cu +(0.394 M) || Cu²+(0.258 M) Cu Cu²+(aq) + 2e → Cu(s); <° = 0.34 V
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V which half reaction takes place at the anode which is the standar cell potential write the balance equation for the overall reaction in acidic sol What is the cell potential for this cell at 25 °C when [Zn²⁺] =...
8. Which of the following statements about the voltaic cell shown below is INCORRECT? Cr(s)|Cr* (aq)||C1,(8)|CI (aq)|Pt(s) (a) Cr(s) and Pt(s) are both electrodes. (b) The double vertical lines, ll, represent a salt bridge. (c) The single vertical line in Cr(s)/Cr represents a phase change. (d) The reaction has three electrodes, Cr(s), Cl(aq), and the inert metal Pt(s).
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)...
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Fe3+(aq) +Al(s) Pb2+(aq) + Au(s) Na+(aq) + Cr(s) Ag+(aq) + Br−(aq) None of the above pairs will react.
Calculate the standard emf of the following cell at 25 degrees C. Cr(s) ⏐ Cr3+(aq) ⎥⎪ Hg22+(aq) ⏐ Hg(l)
On the cell diagram, label (9 pts): • the electrodes (Cr & Cu) • each aqueous solution (Cr(NO3); KNO3; Cu(NO3)2) • anode & cathode • salt bridge (including ions) • the (+) and (-) terminus the direction of electron flow movement of ALL ions where is oxidation occurring, show the process where is reduction occurring, show the process Write the short-hand cell notation (2 pts):
Consider a galvanic electrochemical cell constructed using Cr/Cr3* and Zn/Zn2+ at 25 °C. The following half-reactions are provided for each metal: Cr3+ (aq) + 3 e → Cr(s) Eºred = -0.744 V Zna*(aq) + 2 e Zn(s) Eºred = -0.763 V What is the standard cell potential for this cell?
8) (16 pts) For the following cell diagram, Cr20,2 (aq)IC3+(aq) Cl-(aq)ICl2(8) A. Write the reduction and oxidation half reactions, balance the equation in acidic condition. Combined reaction: B. Determine the standard cell potential E cell Is the reaction spontaneous? C. Once the two hal reaction quotient and Nernst' equation. f cells are connected and allowed to discharge for a while, discuss how cell potential changes F. Calculate the standard free energy change for this reaction. G. Determine the equilibrium constant...