Standard Reduction Potentials at 25 °C Half-reaction Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e-Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Au+ 2Au + Au³+

Determine the cell potential for the following reaction: Hg2+ + 21→ Hg + 12 Given the following standard reduction potentials: Hg2+ + 2 e-→ Hg 2 + 2 e-→21- +0.854 V +0.536 V 0.318 V -0.318 V O-1.39 V O 1.39 V

Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Ch (g) + 2 e–→ 2 CI (aq) 1.360 02(g) + 4 H30*(aq) + 4 e→ 6 H20(1) 1.229 2 H20(1) + 2 e – H2(g) + 2 OH(aq) -0.828 |-0.403 Ca2* (aq) + 2 e" - → Cd (s) A 0.124 M neutral aqueous CdCl, solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: 6H,0 | 4H,0* + 4e Half-reaction at cathode: Cd2+ 2e Cd (b) What is the expected decomposition potential? 2.123 V +

Given the following standard reduction potentials, E°red, which species has the  greatest tendency to be oxidized? S (s) + 2 H+ + 2e−    → H2S (g)            E°red = +0.144 V O2 (g) + 4 H+ + 4e− → 2 H2O (l)         E°red = +1.229 V Sn2+ (aq) + 2e−        → Sn (s)              E°red = −0.137 V   HERE ARE THE OPTIONS: O2 (g) S (s) Sn (s) H2S (g)

Given the half-reactions and their respective standard reduction potentials 1. Cu³+ + 2 e- + Cu+ E; = +1.28 V Cu²+ + e E; = +0.15 V E; = = +0.52 V 2. + Cu+ 3. Cu²+ + 2 e- → Cu(s) = +0.34 V 4. Cu* + e- Cu(s) E calculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II). Cu³+ + e Cu2+ E° = V

Nitesh

Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1 atm) || X3+(1 M) | X(s) If the standard cell emf is minus3.26 V, what is the standard reduction potential at 25oC for X3+ + 3e- → X(s)     -3.26 V 3.26 V 1.36 V 1.90 V -1.90 V

›Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M and [Fe²+] = 0.0100 M. Use the standard reduction potentials in this table. Zn(s) + Fe²+(aq) ⇒ Zn²¹(aq) + Fe(s) E = V

Consider the following standard reduction potentials. O₂(g) + 2H₂O(1) +4 Ca²+ (aq) +2e - 40H (aq) E° = 0.401 V Ca(s) E= -2.868 V E°

Standard Reduction Potentials Sn*(aq) + 2e → Sn²*(s) E° = 0.15 V K"(aq) + le → K(s) E° = -2.92 V |3D Faraday's constant is 96,485 C/mole e's An electric current of 1.00 ampere is passed through an aqueous solution of Ni(NO3)2. How long will it take to plate out exactly 1.00 mol of nickel metal, assuming 100 percent current efficiency? A. 386,000 s B. 193,000 s C. 96,500 s D. 48,200 s