4.(a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, andcalculate the standard emf E° of an electrochemical cell described by the following reaction:2 Na Ba Ba²+ + 2 Na(b) What is n?(c) What is AG° for this reaction at 25°?(d) What is the equilibrium constant for this reaction at 25°?

Answered: 4. (a) Use the standard reduction…

Chemistry

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Qq.49. Subject :- Chemistry
Part IV: Express your answer in three significant figures. Show the complete solution. (8) Calculate the Eºcell for the following electrochemical cell: Pb(s) Pb²+ || Cu²+ Cu(s) (9) Calculate the equilibrium constant at 21°C for the following electrochemical cell: Pb(s) Pb²+ || Cu²+ Cu(s) (10) Calculate the Ecell at 18°C when [Fe²+] = 0.890 M, [Fe³+] = 1.0x102 M, [CI] = 3.02x10³ M, and [Cl₂] = 0.405 M Fe²+ (aq) + Cl2(g) → Fe³+ (aq) + Cl(aq)
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4²+. If a standard hydrogen electrode is used Use the standard reduction potentials shown here to answer the questions. as the cathode, the cell potential, Ecell is found to be 0.080 V at 298 K. Reduction half-reaction E° (V) Cu2(aq) + 2e¬Cu(s) 0.337 Part A 2H+(aq) + 20¬H2(g) 0.000 Based on the cell potential, what is the concentration of Cu2+in this solution? Express your answer to one significant figure and include the appropriate units. Templates Symbols uado redo reset keyboard shortcuts help [Cu² = Value Units
A student wanted to observe the reaction of Fe²+, (aq) V3+ (aq) Fe³+ (aq) + √2+ (aq) using an electrochemical cell. He did the setup and found out that the cell produced a voltage of -1.03V. Assuming standard conditions (298.15 K, 1 atm), which of the following observations would be correct? O a. The standard cell potential is equal to Eº v³+²+ - E°F 3+ Fe / Fe +2 3+ b. The reaction was spontaneous The reaction will proceed without any external power source O d. Exchanging the anode and cathode will make the voltage more negative
Which statement is true regarding the galvanic cell in which an electric current is being produced? Zn²* + 2e¯→Zn E° = -0.76 V Cu2* + 2e¯→Cu E° = +0.34 V V Salt Bridge Zn - Cu ZnSO«(aq) CUSO:(aq) (A) Oxidation occurs at the copper electrode. (B) The mass of the copper electrode is increasing. (C) Zinc ions are produced at the copper electrode. (D) Copper ions are produced at the copper electrode.
Nonmetallic phosphorus can be made by the electrolysis of molten P4010. (a) What mass of P is formed by passing a current of 8.60 A through molten P4010 for 1.30 days? The unbalanced chemical reaction representing this electrolysis is shown below. g of P is formed by this electrolysis. (b) How many minutes are needed to plate out 14.00 g of P from molten P4010 using 8.97 A current? minutes are needed. P4010 → P + 0₂
(a) What type of a battery is lead storage battery? Write the anode and cathode reactions and the overall cell reaction occurring in the operation of a lead storage battery.(b) Calculate the potential for half-cell containing 0.10 M K2Cr207(aq), 0.20 M Cr3+(aq) and 1.0 X 104M H+(aq)The half-cell reaction is K2Cr207–(aq) + 14 H+(aq) + 6e-2 ——–> 2Cr3+(aq) + 7H20(l) and the standard electrode potential is given as E°= 1.33 V.
How many seconds does it takes to produce 5,0 L of aluminum sulfide, Cr2S3 measured at 0.95 atm and 23 °C by electrolysis of molten chromic sulfide, using a current of 1.5 A.
A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.
(a) Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution:Na+(aq) + e-1 ——-> Na(s) E° = – 2.71 VH+(aq) + e-1 ——–> 1/2H2(s) E° = 0.00 VOn the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why?(b) Why does the cell potential of mercury cell remain constant throughout its life?
here is the full question. can you please please not reject it and answer
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous ScCl3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Ch(g) + 2 e → 2 Cl'(aq) 1.360 02(g) + 4 H30*(aq) + 4 e» 6 H2O() 1.229 2 H2O(1) + 2 e– H2(g) + 2 OH (aq) -0.828 Sc*(aq) + 3 e - Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? V +

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