Use the table of standard reduction potentials to select a reducing agent that converts NI2+ to Ni but not Fe2+ to Fe. Standard Reduction Potentials in Aqueous Solution at 25 °C Acidic Solution E (V) HOylaq) +2 H*(aq) +2e2 Hạ0(4) 1.77 Aut(aq) +e- Au(s) 1.68 Au* (aq) +3e - An(e) 1.50 Bre(f) +2e + 2 Br (aq) 1.08 NO, (g) +4H (aq) +3e + NO(g) + 2 H:0(4) 0.96 Ag" (sq) +e - Ag(s) 0.7994 Hz,"(ag) +2e + 2 Hg(4) 0.789 Cu* (aqi +2 - Cula) 0.337 Hg, Cla (a) + 2e + 2 Hg() 0.27 2H* (ag) +2e - Ha(s) 0.00 Sn* (aq) + 2 - Snla) -0.14 N* (aq) + 2e - Ni(s) -0.25 Co* (ag) + 2 - Calu) -0.28 Cd* (aq) + 2e + Cdle) -0.40 C* (aq) +e + *(ag) -0.41 Fe* (aq) +2e + Fe(s) -0.44 Zn* (ag) +2e - Za(a) -0.763 C* (aq) + 2 Cala) -0.91 A* (eq) +3e Al(s) -1.66 Mg* (aq) +2e + Mg(s) -2.37 O zn O cd O Sn O O O

Given the following2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq)         E°cell = 0.73 V and AgCl(s) → Ag(s) + Cl-(aq)          E°= 0.222 V What is the standard reduction potential for X2+(aq)?

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =

Consider the following standard reduction potentials: F2(g) + 2 e - 2 F (aq) E° = +2.87 V Mg2*(aq) + 2 e - Mg(s) E° = -2.37 V Under standard conditions, O Mg(s) is a stronger oxidizing agent than F (aq), and Mg2*(aq) is a stronger reducing agent than F2(g), O F (aq) is a stronger oxidizing agent than Mg(s), and F2(g) is a stronger reducing agent than Mg2*(aq). O F2(g) is a stronger oxidizing agent than Mg-"(aq), and Mg(s) is a stronger reducing agent than F (aq). O Mg2*(aq) is a stronger oxidizing agent than F2(g), and F(aq) is a stronger reducing agent than Mg(s).

Calculate the standard free‑energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this table.   2Au3+(aq)+3Ni(s)↽−−⇀2Au(s)+3Ni2+(aq) Δ?∘=   kJ/mol

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 Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 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: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?

Standard Reduction Potentials (Volts) at 25 °C F2 (g) + 2 e-  2 F- (aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e-  6 H2O(l)  1.229 2 H2O(l) + 2 e-  H2(g) + 2 OH-(aq) -0.828 Fe2+ (aq) + 2 e-  Fe (s) -0.440   A 0.122 M neutral aqueous FeF2 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:     +       +       ->       +       +     Half-reaction at cathode:     +       +       ->       +       +     (b) What is the expected decomposition potential? _______ V

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.