At 25°C, E° = +1.88 V for a cell based on the reaction 3 AgCl(s) + Al(s) 3 Ag(s) + Al3+(aq) + 3 Cl(aq). Find the cell potential E (V) if [Al3+] = 0.20 M and [Cl-] = 0.010 M. Hint: what is the value of Q? Enter your answer in decimal format using two decimal places, (value ± 0.02).

Q: The free energy change for the following reaction at 25 °C, when [Hg²*] = 1.17 M and [Sn²+] =…

A:

Q: Consider the following cell reaction: Co(s)+2 H (? M) Co2*(1.00 M)+ H2(g)(1.00 atm) If the cell…

A: The pH of the acid solution is less than 7 and while of the base is greater than 7. The pH and…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A:

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

A:

Q: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction:  2X(s) +  3Y2+(aq)  →2X3+  + 3Y(s) As the charges are equal on both sides.…

Q: Find the cell potential for the following: Al(s)| Al3+ (1 M) || Fe2+ (1 M) | Fe(s) Given: Al3+…

A: Given: Al3+ (aq) + 3 e- → Al (s) E = -1.662V Fe2+(aq) + 2e- → Fe(s) E = -0.45V

Q: The reaction 2Ag*(ag) + Cu(s) → 2Ag(s) + Cu2+(ag) was used in a galvanic celI. E°=0.46 V for this…

A: Given The redox reaction in the galvanic cell is as follows: 2Ag+(aq) + Cu(s)→2Ag(s) + Cu2+ (aq).…

Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

A: The equilibrium constant K is defined as the ratio of the concentrations of the products to the…

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential (Eᵒcell)…

A:

Q: The standard cell potential E°(cell) is +0.77 V for the redox reaction 2 Fe³⁺(aq) + H₂(g) → 2 H⁺(aq)…

A: Here we are required to find the standard potential for the half reaction.

Q: Consider the following cell reaction: Fe(s) + 2 H+(? M) →→→Fe²+(1.00 M) + H₂(g) (1.00 atm) If the…

A: The given cell reaction is Fe(s)  + 2H+ (? M) →  Fe2+ (1.00 M) + H2 (g) (1.00 atm) The concentration…

Q: Part A For the reaction 2Co (aq) + 2Cl(aq)→2Co² (aq) + Cl₂(g). E=0.483 V what is the cell potential…

A:

Q: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V what is the cell potential at 25 ∘C if the…

A: Given reaction: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)  E∘=0.483 V [Co3+]= 0.896 M [Co2+]= 0.548 M…

Q: Given the balanced electrochemical reaction below (M and N represent generic metals), what is the…

A: The concentration of M3+ can be calculated by using Nerst equation. Nerst equation is given as…

Q: The measured cell potential, Ecell, for the cell shown is -0.3645 V at 25 °C. Calculate the H*…

A:

Q: For the reaction 2Co 3+ (aq)+2Cl − (aq)→2Co 2+ (aq)+Cl 2 (g). E ∘ =0.483 V what is the cell…

A: Given information: Standard cell potential of the cell = 0.483 V Temperature = 25 ℃ Concentration of…

Q: Use the Nernst equation to calculate the cell potentials (in V) of the following cells at 298.15 K.…

A:

Q: Calculate Ecell for the electrochemical cell Ag(s) | AgCl(s) | Cl–(aq, 1.0 M) || Cu2+(aq, 1.0 M) |…

A: The Nernst equation is expressed as: Ecell=Ecell°-0.0591nlogOxidationReduction The reaction that…

Q: The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.87…

A: Consider the temperature of the system is 298.15 K. The concentration of X+ ion in the cathode…

Q: The equilibrium constant, K, was found to be 2.5 x108 at 25°C for the following reaction, 2X(s) +…

A:

Q: The standard cell potential E0 for the cell reaction:     Zn + Cu2+       à      Zn2+  + Cu   is…

A: Given :-  Zn + Cu2+ → Zn2+ + Cu  E°cell = 1.100 V  [Zn2+] = 0.01 M  [Cu2+] = 1.0 M  To calculate :-…

Q: )    Using a table of standard electrode potentials, predict whether the following reactions will be…

A: There is something incorrect in equation of part c so it can't be solved For a spontaneous reaction…

Q: Consider the cell Pt(s)/ H2(g, 1 bar)/NaOH (aq, 0.01m), NaCl (aq, 0.01125m)/ AgCl(s) / Ag(s) 2H₂O +…

A: Recall the cell representation,                           Pt s / H2 g, 1 bar / NaOH aq, 0.01 m,…

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: The standard cell potential E°(cell) is +0.77 V for the redox reaction 2 Fe³+ (aq) + H₂(g) → 2 H(aq)…

A: The standard cell potential E°(cell) is +0.77 V for the redox reaction 2 Fe³+(aq) + H2(g) → 2 H+(aq)…

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)|Cr3*(aq, 1.0 M) ||…

A:

Q: Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:…

A:

Q: Consider the following cell notation and use a Table of Standard Electrode Potentials (Appendix Le…

A: Ecell can be calculated using nernest equation. To calculate Ecell , we would first write a complete…

Q: voltaic cell employs the redox reaction: Au(s) + 3 Na+(aq) → 3 Na(s) + Au3+(aq)    E°cell = -4.21 V…

A: The solution is as follows:

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g)           E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm  P V = n R T  P  = ( n/ V ) R T = c R T  c = P / R T  T ( temperature ) = 25…

Q: Use the Nernst equation to calculate the cell potentials (in V) of the following cells at 298.15 K.…

A: For every concentration cell standard electrode potential (E°) is zero. Because here all electrode…

Q: Calculate the standard cell potential (Eºcell) for the cell shown below. Al (s) | Al³+ (aq)|| Ag+…

A: Conventionally, in a cell notation, anode is written on the left side whereas cathode is written on…

Q: At 298K, a particular voltaic cell contains two electrodes  Al(s) | Al^3+(aq) and Ca(s)| Ca^2+(aq)…

A: The cell given is  Al(s) | Al3+ (aq) and Ca(s) | Ca2+ (aq) From the given reduction reactions of Ca…

Q: following reaction at 298 K: 2H*(aq) + Hg(1) H₂(g) + Hg² (aq) Hint: Carry at least 5 significant…

A: Given is an electrochemical reaction.To find the cell potential and equilibrium constant at 298 K.

Q: Calculate the standard cell potential, E°cell, for the following reaction, and indicate if the…

A: Cu2+ (aq) + Mn2+ (aq) + 2H2O (l) ⇌Cu (s) + MnO2 (s) + 4 H+ (aq)

Q: Calculate the standard potential of this cell: Ni(s) | Ni2+(aq) || Cu2+(aq) | Cu(s). E∘=?

A:

Q: For the following redox reaction calculate the standard cell potential of the reaction.  Redox…

A: We should know the oxidation reaction and the reduction reaction. In Oxidation reaction we have loss…

Q: Calculate the actual cell potential (E) at 25.0 oC for the following redox reaction when the…

A: The question is based on concepts of electrochemistry. we have been given a galvanic cell. we have…

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.20 M and [Pb2+] =…

A: Equilibrium constant can be defined as the ratio of concentration of products to concentration of…

Q: The standard potential for the reaction below is -0.308 V at 25°C. 3 Y+2 (aq)  +2 X (s) → 3 Y (s) +…

A:

Q: Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | Fe3+(aq, 0.100 M), Fe2+(aq,…

A: Answer:- This question is answered by using the simple concept of calculation of cell potential…

Q: Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm) | H+(aq,…

A:

Q: Calculate the standard cell potential (E∘�∘) for the reaction…

A: Kc = 8.30 x 10-3   At standard condition :  Temperature (T) = 298 K  Also, F = Faraday = 96485 C  R…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.