Break the following into half-reactions and calculate the Eo for the reaction: 5 Pb(s) + 5 LiHSO4(aq) + 2 KMnO4(aq) + 11 HCl(aq) ---> 2 MnCl2(aq) + 8 H2O(l) + 5 PbSO4(s) + 5 LiCl(aq) + 2 KCl(aq)

Q: Write the cell reaction and electrode half-reactions and calculate the standard potential of each of…

A: SOLUTION: Step 1:

Q: The following half-reaction AlF63-(aq) + 3e- -->Al(s) + 6F-(aq)         °E = -2,07 V. Calculate…

A:

Q: A voltaic cell is constructed with two Zn2+−ZnZn2+−Zn electrodes. The two cell compartments have…

A: The cell is made up of Zn electrodes only. Hence both oxidation and reduction is happening for Zn…

Q: Calculate an equilibrium constant under standard conditions for the following reaction if the Eºcell…

A:

Q: Two concentration cells are prepared, both with 90.0 mL of 0.0100 M Cu(NO3)2 and a Cu bar in each…

A: Note - Since you have posted a question with multiple sub-parts, we are bound solve only the first…

Q: Iron concentrations greater than 5.4 x 10–6 M in water used for laundry purposes can cause staining.…

A: The solubility product is a type of equilibrium constant whose value is temperature dependent.…

Q: In the standard electrochemical cell, Pt(s)|H2SO3laq), H*(aq), SO4 (aq)||Ag*(aq)|Ag(s), v¥hat can be…

A: In a electrochemical cell representation RHS is cathode s reduction all happen over there, LHS in…

Q: At 25oC, the cell Pt, H2(1atm)| HCl (aq) |AgCl, Ag has an emf of 0.332 at 25oC. What is the pH of…

A:

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: Devise cells in which the following are the reactions and calculate the standard cell potential in…

A: An Electrochemical is made of cathode and anode. In the cell process goes on are: oxidation and…

Q: 7. For each of the following reactions Write the oxidation and reduction half reactions Determine…

A:

Q: 4) Explain the following: Discuss the differences between AG and AG°'; between the relative rates of…

A: Interpretation: We have to explain the followings.

Q: Calculate AG for the following reaction: Mn (s) + Zn²+ (aq) → Mn²" (aq) + Zn (s) 0-8. 10 x 101 J…

A: The given reaction is   Mn(s)  + Zn+2 (aq)  →  Mn+2(aq)   +Zn(s) this is the redox reaction and the…

Q: Which of the following is the oxidizing agent in the following redox reaction? 2KMnO4(aq) +…

A:

Q: Break the following into half-reactions and calculate the Eo for the reaction: 5 Pb(s) + 5…

A: Answer: 1.64 V

Q: Q4:-Put a mark of true or false in front of the following statements and correct the error, if any:-…

A: In an electrochemical cell, both oxidation and reduction reactions takes place. During a redox…

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. He constructs a…

A: The expression (constant) that is only applicable for solutions for partially soluble salts that are…

Q: Give the standard cell potential of the following half reaction: MnO4-(aq) + 5Fe2+(aq) + 8H+(aq) →…

A:

Q: The following soluble salts are strong electrolytes. For each, write a balanced equation for their…

A: balanced equation for their dissociation in water. half reaction : Fe(NO3)2(aq) →Fe2+(aq) +…

Q: (i) Pt(s) + 2 NH3(aq) + 2 CI ( (aq) cis-[PtCl₂(NH3)2](aq) + 2 e¯ E° = 0.274 V The likely cathodic…

A:

Q: Consider the cell diagram for an electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) |…

A: For the electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) | Pt having E = 1.40 V , we…

Q: Calculate the biological standard Gibbs energies of reactions of the following reactions and…

A: SOLUTION: Step 1: (a). the oxidation number of each oxygen atom changes from 0 on the left to the -2…

Q: Calculate the standard cell potential, standard free energy change, and equilibrium constant for the…

A:

Q: Calculate the pressure of hydrogen required to stop corrosion of cadmium at 25 °C in deaerated…

A: Solution Many ionic compounds don't totally dissolve in water. once extra to water, a number of the…

Q: A fuel cell differs from a battery because the current is being generated from a reduction-oxidation…

A: When a weak acid dissociates it does not undergo complete dissociation. So, when phosphoric acid…

Q: Q4:-Put a mark of true or false in front of the following statements and correct the error, if any:-…

A: In an electrochemical cell, both oxidation and reduction reactions takes place. During a redox…

Q: A 17.1769 mL sample of an acid was titrated with electrogenerated OH-. It took 617s at a constant…

A: Given: Volume of acid solution = 17.1769 mLCurrent = 0.216 ATime = 617 seconds

Q: For the reagents below: - Write the redox half-reactions involved for each compound - Write the…

A:

Q: A 220 mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A:

Q: What volume of hydrogen – at 1 atm and room temperature - was produced during that time?

A: Oxidation is happened in anode, while cathode, reduction is taking place.  The stoitchiometric…

Q: Calculate the standard Gibbs energies at 25 °C of the following reactions from the standard…

A: Since we answer only upto 3 sub-parts, we'll answer first three. Please resubmit the question…

Q: A student measures the potential of a cell made up with 1 M CuSO4 in one solution and 1 M AgNO3 in…

A:

Q: Tell weather the following redox reactions is spontaneous or not. With explanations/solution 3+ C.…

A: Redox reaction are those in which both oxidation and reduction reaction occurs simultaneously.

Q: For the following reactions, (i) write the half-reactions, (ii) write a balanced equation for the…

A: Redox reaction- the reaction in which oxidation and reduction takes place simultaneously called as…

Q: For each of the following; a. Write the overall cell reaction/ cell representation b. Calculate…

A: 1. Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) Writing the overall cell reaction/cell representation

Q: What is the cell diagram for the reaction: 2A9CI(s) + H2(g) → 2Ag(s) + 2H*(aq) + 2C1 (aq)…

A:

Q: Which one of the following reactions (as written) should proceed spontaneously under standard…

A: Cell potential is calculated as E°cell = E°cathode - E°anode And is E°cell is positive then the cell…

Q: For the reaction NI2*(aq) + 2FE2*(aq) – NI(s) + 2FE3*(aq), the standard cell potential Ecell is…

A: The answer to this question is given below:

Q: Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should…

A: A question based on electrolysis that is to be accomplished.

Q: Give the standard cell potential of the following half reaction:   Cr2O72-(aq) + 3H2O2(aq) +…

A: Cr2O72- + 3H2O2 + 8H+ .....> 2Cr3+ + 3O2 + 7H2O In this redox reaction, Cr is reduced from +6 to…

Q: How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis  W= (E×i×t)/96500 W= mass of a…

Q: Devise cells in which the following are the reactions and calculate the standard cell potential in…

A: a) 2Na + 2H2O ------> 2NaOH + H2     2Na ----> 2Na+ + 2e-               E = 2.71 V     2H2O +…

Q: 4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the…

A:

Q: A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O*(aq) → Pb²+ (aq) +…

A: Given data are  cell potential = 0.22V Cl- = 0.15M P H2 = 1.0 Atm. Pb2+ = ? ∆E = ? solubility…

Q: 9. Using the appropriate half-cell reactions, and assuming y. 1, calculate the solubility product of…

A: The dissociation reaction of AgCl in water is: AgCl (s) ↔ Ag+ (aq) + Cl- (aq) For this reaction,…

Q: What is the Nernst expression corresponding to the following half-reactions: Zn2+ + 2e- ⇌ Zn(s) Fe3+…

A: Since your question has multiple sub-parts, we will solve only first three sub-parts for you. If you…

Q: Balance the following reaction in basic solution. Ag(s) + Zn?+ (ag) → Ag,0(ag) + Zn(s) Fill in the…

A: The chemical equations should be balanced in accordance with the law of conservation of mass. This…

Q: an electric current is passed through two electrolytic cell connected in series (same amount of…

A: Reactions in which a chemical species loses electrons is called oxidation reactions. Reactions in…

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.