Determine theoretical cell potential of the following celli Pt/Fe 3+ (1.50M), Fe2+ (0.01 M/ Cr3+ (0.10...
What is the cell potential for the following reaction when [Fe2+] = 0.25 M and [Fe3+] = 0.01 M? You may use the standard reduction potentials on your data sheet. Fe(s) + 2 Fe3+(aq) → 3 Fe2+(aq)
Calculate the theoretical cell potential for each of the following cells. Is the cell, as written, galvanic or electrolytic? a. Pb | PbSO_4 (sat'd), SO_4^2- (0.200 M) || Sn^2+ (0.150 M), Sn^4+ (0.250 M)|Pt b. Pt |Fe^3+ (0.0100M), Fe^2+ (0.00100M) || Ag^+ (0.200M), CuI (sat'd) |Cu d. Pt | UO_2^2+ (0.0100 M), U^4+ (0.0100 M), H^+ (1.00 times 10^-6 M) || AgClO (sat'd), KCI (1.00 times 10^-4 M) |Ag
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...
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) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+ = +0.771V, Eo Ce4+/Ce3+ = + 1.44V a) Draw the complete cell represented by the above line diagram and label all the components. b) Write the half-cell reactions and complete redox reaction of the cell. c) Calculate the standard cell potential. d) Calculate the cell potential at the non-standard conditions provided above. e) Was the cell reaction spontaneous?
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...
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) |...
For the electrochemical cell, Fe(s)| Fe2+ (aq)|| Cu2+ (aq)| Cu+ (aq) | Pt(s), determine the equlibrium constant (Keq) at 25°C for the reaction that occurs.
What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 87 ∘C when [Fe2+]= 3.00 M and [Mg2+]= 0.110 M .
What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 81 ∘C when [Fe2+]= 3.80 M and [Mg2+]= 0.310 M