Question-1: Consider the cell, Zn(s)|ZnCl2(0.0020 mol kg)|Hg,Cl2(s)|Hg(1l), for which the cell reaction is Hg,Cl2(s) + Zn(s) → 2Hg(1) + 2CI¯(aq) + + Zn²*(aq). Given that E°(Zn2+,Zn) = -0.7628 V, E°(Hg2Cl2,Hg) = +0.2676 V, and that the cell potential is +1.2272 V. (a) Write the Nernst equation for the cell. (b) Determine the standard cell potential. (c) Determine A,G, A,Gº, and K for the cell reaction.

How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to FeSO4? What is the volume (in cm3) of 0.10 M K2Cr2O7 that can be reduced to chromic sulfate, Cr2(SO4)3, by the same quantity of electricity?

Give the standard line notation for each cell. (a) 2 IO3¯(aq) + 10 Cr²+ (aq) + 10 H+ (aq) ⇒ 10 Cr³+(aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Cr²+ (aq), IO3¯(aq), H+ (aq) || Cr³+ (aq), I2 (aq) | Pt(s) Pt(s) | Cr³+ (aq), I2 (aq) || Cr²+ (aq), 103¯(aq), H+ (aq) | Pt(s) Pt(s) | IO3¯(aq), H+ (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) Pt(s) | Cr²+ (aq), Cr³+ (aq) || IO3¯¯(aq), H† (aq), I₂ (aq) | Pt(s) (b) (c) (d) Co(s) + 2 Ag+ (aq) ⇒ Co²+ (aq) + 2 Ag(s) Co(s) | Ag+ (aq) || Co²+ (aq) | Ag(s) (aq) || Ag* (aq) | Co(s) Ag(s) | Co²+ 2+ Ag(s) | Ag+ (aq) || Co²+ (aq) | Co(s) 2+ Co(s) | Co²+ (aq) || Ag+ (aq) | Ag(s) H2O2(aq)+2 H*(aq)+2e O₂(g) + 2 H+(aq) + 2 e¯ → H2O2(aq) Pt(s) | H₂O₂ (aq) | 02 (9) || H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq) | Pt(s) Pt(s) | H₂O2 (aq), H+ (aq) || O2(g) | H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | O2(g) | H₂O2 (aq), H† (aq) || H₂O2 (aq), H† (aq) | Pt(s) 00 Mn²+ (aq) + 2 e → Mn(s) → 2H,O(l) 3+ Fe³+ (aq) + 3 e → Fe(s) Eº E° -1.18 V 3+ Fe(s) | Fe³+ (aq) || Mn²+ (aq) | Mn(s) Fe(s) | Mn²+ (aq)…

(a) In the electrolysis of aqueous Na2C204, how many liters of H2(g) (at STP) are generated by a current of 82.6 A for a period of 54.0 min? The unbalanced chemical reaction representing this electrolysis is shown below. Na2C204(aq) + H20(1) → CO2(g) + H2(g) + NaOH(aq) liters of H2(g) is generated by this electrolysis. (b) How many moles of NaOH(aq) are formed in the solution in this process? moles of NaOH(aq) are formed.

Consider the same diagram of a galvanic cell as in previous question, conventional current anode X X+ (aq) (C) 0.76 V (D) 0.91 V A e flow Salt bridge Y+ (aq) cathode where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq). Given the following electrode potentials: Ag (aq) + e-> Ag(s); E° = 0.80 V Ni²+ (aq) + 2e --> Ni(s): E = -0.23 V What is the Ecell at 25°C when the electrolyte concentrations are [Ag*] = 1.3 x 10-5 M and [Ni²+] = 0.10 M. (A) 1.15 V (B) 1.30 V

Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation:

Cu(s)||Cu2+(aq, 0.0155 M)‖‖Ag+(aq, 3.50 M)||Ag(s)Cu(s)⁢|Cu2+⁢(aq, 0.0155 M)‖Ag+⁢(aq, 3.50 M)|Ag(s)   net cell equation: Cu+2Ag+⟶Cu2++2AgCu+2⁢Ag+⟶Cu2++2Ag   Calculate ?∘cell, Δ?∘rxn, Δ?rxn, and ?cell at 25.0⁢ ∘C, using standard potentials as needed. ?∘cell=   0.46 V Δ?∘rxn=  -88.76    kJmol Δ?rxn=       kJmol ?cell=      V I just need help with the last 2

3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)

9:-0 electrode is called (a) anode, oxidation (b) anode, reduction O (c) cathode, oxidation (d) cathode, reduction (e) cannot tell unless we know the species being oxidized and reduced. The standard electrode potentials of the electrodes Cu+ | Cu and Ag+ | Ag are 0.337 V and 0.7991 V. What would be the concentration of Ag+ in a solution containing 0.06 M of Cu*+ ion such that both the metals can be deposited together. Assume that activity coefficients are unity and both silver and copper do not dissolve among themselves. 12.98x10-8 mole/dm-3 15.22x10-8 mole/dm-3 10.37x10-8 mole/dm-3 The standard electrode potentials of the electrodes Ag+ | Ag and Fe+, Fe* | Pt are 0.7991 V and 0.771 V respectively. Calculate the equilibrium constant for the reaction

Give the e.m.f. and the overall reaction of the following cell: Pt(s) | H2 | H*(aq) | Ag*(aq) | Ag(s) Calculate the value of E° for each of the following reactions. Decide whether each is product-favored in the direction written. (a) 21(aq) + Zn²*(aq) – I:(s) + Zn(s) (b) Zn*(aq) + Ni(s) →Zn(s) + Ni²*(aq) (c) 2 C1 (aq) + Cu"(aq) →Cu(s) + Cl2(g)