Using 1.0 A of current for 60 s, what metal solution will deposit the highest mass of metal ? F=96470 J/V x mol e- = 96470 A x s/mol e- = 96470 C/mol e-   a. depositing Fe from Fe(NO3)2 b. depositing Fe from Fe(NO3)2 c. Depositing Cu from CuNO3 d. Depositing Cu from Cu(NO3)2

Q: Cr2O7 2- (aq) + 14H+  6e- ---> Cr3+(aq) + 7H2O(l) Ered = 1.33V Cu2+(aq)  + 2e-  --> Cu(s) ?°red =…

A: For the given cell reaction the reduction potential of the electrodes is as follows: Cr2O7 2- (aq) +…

Q: Al+3 + 3e --> Al Eo = -1.66 V   Ti+2 + 2e --> Ti Eo = -1.63 V        Which option is correct for…

A: Given: Al+3 + 3e --> Al.          Eo = -1.66 V Ti+2 + 2e --> Ti           Eo = -1.63 V

Q: Which of the following reactions is NOT spontaneous under standard conditions? Select one: a.…

A: Answer:- These question are answered by using the simple concept of electrochemistry which…

Q: A solution containing Pt*+ is electrolyzed with a current of 4.10 A. How long will it take to plate…

A: W = E i t /F W = mass to be deposited E = equivalent Weight i = current in ampere t = time in second…

Q: Given: Cr3+(aq) + 3e– ----> Cr(s); E° = –0.74 V Ag+(aq) + e–   --------> Ag(s); E° = 0.80 V What…

A: Answer:

Q: 7) A galvanic cell is being made of iron & chromium. The standard reduction potentials are: Fe^2+…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

Q: What is the standard cell potential of a cell created using a cadmium electrode in 0.30 M…

A:

Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

A: Here we are required to find the cell potential of the given two electrochemical reaction

Q: (a) The half-reaction for formation of magnesium metalupon electrolysis of molten MgCl2 is Mg2+ + 2…

A: (a) The value of current for formation of magnesium is 60.0 A. The value of time taken for formation…

Q: Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu2 (aq) (x M)| Cu(s) Cd2* + 2e Cd E° = -0.40 V Cu2*…

A: The half-cell reactions are : Cd2+  +  2e-  →  Cd                E°=-0.40 VCu2+  +  2e-  →  Cu…

Q: Consider the electrolysis of a solution that is 1.0 x 10-3 M in Ag2SO4 and 1.0 x 10-1 M in ZnSO4…

A: Given, Molarity of Ag2SO4 = 1× 10-3 M  Then, normality = 2 × Molarity…

Q: Consider the electrochemical cell described by the following reaction at 310 K. The measured cell…

A: Cell potential is  0.242V , R=8.314J/mol-K, F= 96485C/mol , E° (reduction)= -0.17V, E°(oxidation)=…

Q: Ni+ (ag) + Cd(s) → Ni(s) + Cd?+ (aq) E cell = +0.15 V Under standard conditions, a Ni-Cd galvanic…

A: A Galvanic cell is made up of an anode and a cathode.   Reduction reaction occurs at cathode whereas…

Q: olution is: .K. c) 144727.5 J.mol.K A concentration cell is constructed by placing identical Ni…

A: In a concentration cell, electrolytic concentrations in anode and cathode are taken such that cell…

Q: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: The galvanic cell formed will be such that the standard cell potentialof the cell is positive.…

Q: Based on the table of reduction half- potentials, which is most likely to be reduced? Standand…

A:

Q: Consider the following standard reduction potentials: Fe3+ (aq) + e MnO4 (aq) + 8 H*(aq) + 5e → Mn2+…

A: In this question, we will see the strongest oxidizing agent.  You can see below.

Q: Consider the cell: Cd(s) | Cd2+(aq) (0.035M) || Cu2+(aq) (x M)| Cu(s) Cd2+ + 2e → Cd E° = -0.40 V…

A: In this given question we want to calculate the concentration Cu2+ so we can use the Nernst equation…

Q: a. Calculate the equilibrium constant for the following reaction at 25°C: Ag* (aq) + Fe2+ (ag) →…

A:

Q: 21. How many grams of Cu will be plated out by a current of 2.3 a applied for 25 minutes to a 0.50 M…

A: According to the Faraday's law of electrolysis The amount of an element deposited at an electrode is…

Q: At 25 °C, based upon the overall reaction                 Zn2+(aq) + 2 Fe2+(aq) ⟶ Zn(s) + 2…

A: The expression for the Nernst equation is shown below: Where; Ecell = cell potential E0cell =…

Q: The following electrochemical cell has a cell voltage of 0.033 V at 25oC and 1.00 atmosphere…

A:

Q: A solution containing Pt*+ is electrolyzed with a current of 5.20 A. How long will it take to plate…

A: Using the formula for mass deposition.  Mass deposited = Zit/nF Where,  Z = molar mass = 195.084…

Q: A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3)2(aq),…

A:

Q: i) Consider an electrochemical cell involving Nickel and Copper. Ni2- (aq) + 2e- - Nia E° = -0.25 V…

A: When we have to decide which acts as anode and which acts as cathode. Simply look at the reduction…

Q: i) Consider an electrochemical cell involving Nickel and Copper. Ni2* (a0) + 2e- → Nis E° = -0.25 V…

A: On the basis of Reduction potential, the substances which have the lower reduction potentials are…

Q: 24. A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(N03)2(aq),…

A: Since the concentration of ions are 1 M that is standard concentrations Hence the cell potential…

Q: An aqueous copper(II) sulfate solution is electrolyzed for 30 minutes. A 3.0 ampere current is used.…

A:

Q: A solution containg 75.0 mg copper was electrolyzed at a constant current of 0.250 A, causing…

A: Faraday's first law :  The amount of substance deposited is directly proportional to quantity of…

Q: A steady current of 5 A  is maintained for 120 seconds in CuSO4 solution. How much Cu is deposited…

A:

Q: Consider the following standard reduction potentials in acid solution: E (V) -1.66 A13+ + 3e - Al(S)…

A: Consider the given standard reduction potential in acid solution is as follows; Al3+  +   3e-    →…

Q: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: The Nernst  equation is given as :

Q: If a piece of silver is placed in a solution in which [Ag*] = [Fe2*] = 1.00 Mat STP, what is Ecell…

A: In the given electrode reactions the silver metal is oxidized into the silver ion and the iron (II)…

Q: What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuS04 solution in one…

A: Provided time(t)= 1 hours Provided time(t)= 3600 second Provided Molar mass of Cu=63.5g/mol…

Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) the ion concentrations are [Cu2+]…

A: Answer: Ecell =1.045 V

Q: Pt(s) | H,(g, 0.703 atm) | H* (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction…

A:

Q: Question six in photo

A: When Cobalt metal dissolves in nitric acid, Cobalt nitrate is obtained with the evolution of…

Q: Pb2+ + 2e– → Pb ε° = –0.13 V Cu2+ + 2e– → Cu ε° = +0.34 V If the Pb2+ and Cu2+ are each 1.0 M,…

A: This problem is based on Nerst Equation For which, first we need to calculate the E°cell E°cell =…

Q: Consider the battery represented by the following notation. Ni(s) | Ni²*(aq) || Ag*(aq) | Ag(s)…

A:

Q: 1.How many grams of NaCl is present on 5.0 mL of 1.0 % m/V NaCl solution?

A:

Q: Consider an electrochemical cell involving Copper and Iron.    Cu2+(aq) + 2e- → Cu(s)     Eo = 0.34…

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Q: 5. Consider the reaction, Li+28r → Brz+Li What is the standard potential for this reaction? For the…

A: 6) Given that: Current (I) = 5.2 A Time (t) = 8 s Charge (Q) = ?

Q: How much time (in s) is needed to deposit 0.0125 g of chromium from a solution of Cro+ with a…

A: Given Weight = 0.0125 Current = 1.5 A F = 96500 A-s/mol e- Molar mass of chromium = 52 g

Q: A solution containing Pt4+  is electrolyzed with a current of 4.30 A. How long will it take to plate…

A: The solution is as follows :

Q: 4. Calculate the emf of the cell Co|Co2+||Ni2+|Ni If the concentrations are [Ni2+] = 1.0 M and…

A:

Q: Predict whether the following reactions would occur spontaneously in aqueous solution at 25°C.…

A: standard conditions are given: Temperature = 25° C Initial concentration of all the dissolved…