Please show all work step by step and final answer.
The given reaction is
Hence, using Nernst's equation, we can write the cell potential of the reaction as
Where Q is the reaction quotient.
Now, as the reaction reaches equilibrium, the reaction quotient Q become equal to equilibrium constant K.
We know that the standard free energy change of the cell reaction
The standard free energy change is also related to the equilibrium constant K as
Hence,
Now, substituting the value above in the Nernst's equation
Hence, the cell potential of the cell at equilibrium is 0 volts.
Please show all work step by step and final answer. Cell Potential at Equilibrium For a single galvanic cell based on t...
Please show all work step by step and final answer. Cell Potential at Equilibrium For a single galvanic cell based on the (unbalanced) reaction: Ag+ (aq) + Zn(s) = Zn2+(aq) + Ag(s) What is the cell potential when the cell reaches equilibrium? Submit Answer Tries 0/5
Please show all work step by step and final answer. Using tabulated standard reduction potentials from your text, calculate the standard cell potential, Eºcell (always positive for a galvanic cell), based on the following reaction: Cu2+(aq) + Mg(s) = Mg2+ (aq) + Cu(s) Eºcell = cf Table A5.5, p A24 Zumdahl "Chemical Principles" 8th ed. 1pts Submit Answer Tries 0/5 A galvanic cell based on the above reaction is constructed according to the generic sketch of a galvanic cell shown...
Please show all work step by step and final answer. Reference Electrodes The Eº value for the following reaction is 0.446 V relative to the standard hydrogen electrode (SHE): Ag2 CrO4(s) + 24 + 2Ag(s) + Cro42 (aq) A chemist wishes to determine the concentration of Cro42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a silver wire coated with Ag Cro4 and...
What is the standard potential of the galvanic cell that utilizes the following reaction (unbalanced). AuCl2-(aq) + Cu(s) ⇌ Au(s) + 2Cl-(aq) + Cu2+(aq Please show your work, thanks!
Part II. Answer the following questions. Please show ALL your work when needed. 1. Calculate the equilibrium constant from the cell potential: (6 points) Zn(s)[Zn2+ (aq)||Cu2+ (aq) Cu(s) Zn2+ 2e Zn(s) E = -0.76V Cu?"(aq) + 2e → Cu(s) E = 0.34V
Please help me solve this An electrochemical reaction occurring in a galvanic cell is expressed using the standard cell notation: Zn(s) Zn2+ (aq) || Ag (aq) | Ag(s) The standard reduction potentials for the half-cell reactions are as follows: Zn2+(aq) + 2e_? Zn(s) E o=-0.76 V Ag (a)eAg(s) E +0.80 V Which of the following statements is correct regarding this electrochemical cell? A. Agt is reduced at the cathode; Zn is oxidized at the anode. B. Edell = +1.56 V...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
Please explain what you do and why. A galvanic cell is setup with the following two half-cells: A 250.0 mL solution of 0.15 M aluminum nitrate with a platinum electrode. A 250.0 mL solution of 0.85 M cobalt(II) nitrate with a cobalt electrode. a) Determine the cell potential that will be initially measured for this galvanic cell b) How much mass is gained/lost by the cobalt electrode after the cell reaches equilibrium? c) If it takes this galvanic cell 2.00...
Please show all work step by step and final answer. Relative Reduction Potential Assuming standard conditions,, and considering the table of standard reduction potentials for half-reactions, given in your text, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6" Cr2+ Pb2+ (acidic half-cell solution) Cu Zn Ag Ca Tries 0/5 Submit Answer
Please show all work to get final answer and circle correct answer. Thanks 9. (8 pts) Consider the following oxidation-reduction reaction occurring in acidic solution: Zn(s) + NO3 (aq) → Zn²+ (aq) + N2O(g) Write out and balance the reduction half-reaction involving NO3 and N20 below. 10. (4 pts) Use the table of data to find the standard cell potential (E cell) for the voltaic cell based on the reaction below. Show your work to receive full credit. Half-reaction Cr3+...