Given the reaction Sn(s)+ 4OH-(aq)+ 2Pt2+(aq)⇌SnO2(s)+ 2H2O(l)+ 2Pt(s)for which E°cell= 2.13 V, what is the value of Ecell, in volts, when the [OH-] = 1.00x10-5M and [Pt2+] = 3.00x10-3M at 25.0 °C?
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Given the reaction Sn(s)+ 4OH-(aq)+ 2Pt2+(aq)⇌SnO2(s)+ 2H2O(l)+ 2Pt(s)for which E°cell= 2.13 V, what is the value...
Conceptual: Consider a Sn(s)|Sn2+(aq) || Cu2+(aq)|Cu(s) cell. If the Sn2+ concentration is increased, what will happen to the measured Ecell value? • Calculation, full-reaction Nernst equation: Use the full Nernst equation to calculate Ecell for the conditions described… • Easier: Ni | Ni2+(0.300 M) || Cu2+(0.002 M) | Cu • Harder: Al | Al3+(0.002 M) || Cu2+(4.00 M) | Cu • Calculation, half-reaction Nernst equation: Use the Nernst equation to calculate E at pH 3.00 and [Cl- ] = 0.0035...
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Half-Reaction
E
°
(V)
Ag+ (aq) + e− → Ag (s)
0.7996
Al3+ (aq) + 3e− → Al (s)
−1.676
Au+ (aq) + e− → Au (s)
1.692
Au3+ (aq) + 3e− → Au (s)
1.498
Ba2+ (aq) + 2e− → Ba (s)
−2.912
Br2 (l) + 2e− → 2Br− (aq)
1.066
Ca2+ (aq) + 2e− → Ca (s)
−2.868
Cl2 (g) + 2e− → 2Cl− (aq)
1.35827
Co2+ (aq) + 2e−...
Consider an electrochemical cell based on the following reaction: Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq) + H2(g) All dissolved species are at 2.5 x 10-3 M; pressure of H2 is 1 bar (standard state) Use the Nernst equation to calculate E.
1) Given the reaction Cd(s)+Ni2+(aq)------>Cd2+(aq)+Ni(s) Calculate the equilibrium constant (K). Ecell of +0.350 V and at 25.0 celsius 2)If 75.0mL of 0.195 M Hbr is combined with 75.0mL of 195M Ca(OH)2 at 25.0 celsius calculate the pH of this solution
1--What is E°cell for the following hypothetical reaction exactly as written (in volts), given the standard electrode potential (E°) values below? X(s) + Y2+(aq) → X2+(aq) + Y(s) X2+(aq) + 2 e- → X(s) E° = -0.69 V Y2+(aq) + 2 e- → Y(s) E° = -2.45 V 2--In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Pt(s)|H2(g)|H+(aq)|| Ag(s)|Ag+(aq) Select one...
1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). A. If the concentration of Sn2+ in the cathode compartment is 1.30 M and the cell generates an emf of 0.25 V , what is the concentration of Pb2+ in the anode compartment? B. If the anode compartment contains [SO2−4]= 1.30 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4? 2. A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). A. What is the emf...
At 58.0 ∘C , what is the maximum value of the reaction quotient, Q, needed to produce a non-negative Ecell value for the reaction SO42−(aq)+4H+(aq)+2Br−(aq)⇌Br2(l)+SO2(g)+2H2O(l) In other words, what is Q when Ecell=0 at this temperature? I found that Ecell = 0.87 V and n= 2 −nF(Ecell−E∘cell) / 2.303RT = 2×96485 (0+0.87)/2.303×8.314×331.0 log q = -26.49 I need Q without log
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?
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.
A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2VO+2(aq)+4H+(aq)+Fe(s)->2VO+2(aq)+2H2O(l)+Fe+2(aq) Suppose the cell is prepared with 3.82 M VO+2 and 1.96 M H+ in one half-cell and 4.70 M VO+2 and 6.88 M Fe+2 in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.