14.58 Complete and balance the following oxidation-reduction reactions, assuming they occur in acidic solution. (a) C20;-(aq)+MnO;(aq)* CO(g)+Mn²*(aq) (b) CIO7(aq)+Cl¯(aq)* Cl2(aq) (c) S203(aq)+I½(aq) so;"(aq)+I¯(aq)

Q: An aqueous solution of copper sulphate, CuS04 was electrolysed between platinum electrodes using a…

A: a) The solution is containing CuSO4 solution with Cu2+ ions. Since a cathode, the reduction reaction…

Q: Give the standard line notation for each cell. (а) 2 IO3 (aq) + 10 Fe?+ (aq) + 10 H* (aq) = 10 Fe…

A: Single vertical line indicate phase boundary, double vertical line is salt bridge.Left of the salt…

Q: Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). How many moles of…

A: In the given reaction we can see that the Ag+ is being reduced to the Ag and Fe2+ is being oxidised…

Q: The permanganate ion, MnO4- , is a common oxidizing agent. What is the standard potential of the…

A: Standard reduction potential is the potential difference occurring between the cathode and anode. It…

Q: The thermodynamic solubility product of AGCN is 6.0×10¬17.

A: Ksp,AgCN=6.0×10-17

Q: If you complete and balance the following equation in acidicsolutionMn2+(aq) +…

A: …

Q: Complete and balance the following oxidation-reduction reactions, assuming they occur in basic…

A:

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The answer is as follows:

Q: Consider the following galvanic cell reaction at 25 oC, 4 Cr2+(aq) + O2(g) + 4 H3O+(aq) → 4 Cr3+(aq)…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: aq) + Clo (aq) – I3 (aq) + Cl (aq) oW DO WE GET THERE? liminate as many H20 molecules as possible.…

A:

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: For a spontaneous reaction, the cathode must have higher electrode potential than the anode. The…

Q: (Show your complete solution) For each of the following redox reactions, (i) Write the…

A: Redox reaction is a reaction in which oxidation and reduction take place simultaneously. In this…

Q: What is the concentration of hydronium ions in (a) a solution that is 0.12 M HBRO(aq) and 0.160 M…

A: Buffer solutions are the solutions that resist a small change in pH when some amount of acid or…

Q: b. The following equations represent various acid/base reactions. Complete and balance each…

A: According to Bronsted and Lowry concept an Acid is a substance that has the tendency to donate a…

Q: Complete and balance the following half-reaction in basic solution S2 (aq) → SO2(g)

A: Given unbalanced half reaction is,  S2– (aq)→SO2 (g)

Q: Which of the following reactions has the largest equilibrium constant (K) at Standard Conditions?…

A: Keq = [Product]/[Reactant] However, the concentration of liquid and solid is taken as 1.

Q: Calculate the equilibrium concentration of Ag*(aq) in a solution that is initially 0.140 M AgNO3 and…

A: The correct answer is given below

Q: 14.56 Complete and balance the following oxidation-reduction reactions, assuming they occur in basic…

A:

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: O What is E°(cell) for the cell Pt(s) | Ce³(aq), Ce(aq) || Br₂(aq), Br(aq) | Pt(s)? What is Eº(cell)…

A:

Q: Complete and balance the following equations for reac- tions taking place in basic solution. (a)…

A: Redox reactions are the reactions in which oxidation and reduction occur simultaneously. Balancing…

Q: Assume the pe of the surface water of a lake is controlled by the O,/H,O half-reaction. What would…

A: When two half cell potential is given we can calculate nernst potential. The two half cell…

Q: Copper from a 200.0 mL solution of copper (II) sulfate is plated on to the cathode of an…

A:

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, . The reaction that occurs…

A: Give that: the reaction of anode is: 2Cl- (aq) →Cl2 (g) + 2e- Mass of Cl2 produced, w =182 g, time…

Q: 4. Write the overall net ionic equations for the following voltaic cells: (a)…

A: (a)  Given,  Zn(s) Zn²+ (aq)||Fe²+ (aq)|Fe(s) Anode reaction;  Zn(s) -----> Zn²+(aq) + 2e-…

Q: Complete and balance the following redox reaction in basic solution Cr,0, (aq) + 1,(s) Cr* (aq) +…

A: Balance the half redox reaction using the steps At last add both and cancel out common term.  And…

Q: Write balance redox reactions, for the following short hand notations: (a) Cu(s) | Cu²“(aq) ||…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: At 18°C a 0.001-M aqueous solution of potassium hydrogen carbonate, KHCO3 , conducts a current in a…

A: Potassium bicarbonate dissolve in water. It dissociate into water to produce potassium ion ( K+)…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: The salt given is KC3H5O3.

Q: Complete and balance the following equations for reac- tions taking place in acidic solution. (a)…

A: Redox reactions are the chemical reactions in which gain of electron(reduction) and loss of electron…

Q: (7): Calculate the pH and percent deprotonation of 0.10 M acetic acid CH3COOH (aq)(use Table 15.5 to…

A: Calculation for finding out hydrogen ions:

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A:

Q: The Haber process is the principal industrial route for convertingnitrogen into ammonia:N2(g) + 3…

A: It is given that nitrogen is reacting with 3 moles of hydrogen to give 2 moles of ammonia and the…

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.