How long would it take (in minutes) to reduce 1 mole of each of the following ions using the current indicated? (Ampere (A) = Coulomb/second (C/s), I = C/s, F= 96500 C/mol e-) (C = Charge unit Coulomb, n = electron mole number)    Q=I×t=n×F (a) Fe3+ , 2.344 A (b) Cu2+ , 25.260 A

Q: How long would it take to titrate 1.00 mmol H2S with a current of 100.0 mA?

A:

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

Q: Multiple Choice For each pair of standard cell potential and electron stoichiometry values below,…

A:

Q: 5. For the following reaction at 25 °C, 5FE2+ *(aq) + MnO4 (aq) + 8H"(aq) = 5Fe*(aq) + Mn²*(aq) +…

A: Given :  [Fe+2] = 0.50 M  [Fe+3] = 0.10 M  [MnO4-] = 0.025 M  [Mn+2] = 0.015 M pH = 7.00  => [H+]…

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given, Current = 62.7 A Time = 81.9 min NaNO2 (aq) + H2O (l)     NO (g) + O2 (g) + NaOH (aq)…

Q: Half-reaction E° (V) 1(s) + 2e → 21°(aq) 0.535V 2H*(aq) + 2e H2(g) 0.000V Cr*(aq) + 3e¯…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

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

A: EFM of the cell is calculated by using below formula,

Q: Complete and balance the following half-reaction in basic solution. Be sure to include the proper…

A: Answer:A chemical reaction in which oxidation and reduction of species takes place simultaneously is…

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

A:

Q: 3(a) Balance the following oxidation-reduction equation. NH3(g) + O2(g) → NO(g) + H2O(l) If Br2 is…

A: a) The given reaction is, NH3(g) + O2(g) ---> NO(g) + H2O(l)

Q: The II, III, and IV oxidation states of Mn are related thermodynamically by these equilibria in acid…

A: Given:Determine the standard electrode potential of the couple.The standard electrode potential…

Q: at a temperature of 25 ° C the galvanic element Pt | ClO3- 0,001M, Cl- 0,01M pH = 3 || Mn2 + 0.0001M…

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Q: Which species functions as the oxidizing agent in the following reduction-oxidation reaction: 5…

A: The Correct option is MnO-4 (aq).

Q: How many Seconds are reQuircd to deposst o.2859 Or Cadmium metal from a Solutior that Contams cazt…

A: By Faradays law of electrolysis; W/E = It/F where, W = mass of substance deposited E = equivalent…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A:

Q: (a) The cell potential for the following electrochemical cell at 25°C is 1.00 V. Pt(s) |H2 (g, x…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: The eqalibrium constant, K, for a redox reaction. 18 related to the standard potentials to, by the…

A: Given: Equilibrium constant for the reaction = 9.10 × 10-4  And the reaction is X (s) + Y+ (aq) → X+…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq)…

A:

Q: Q3: A- Calculate the Molality of a solution containing 5.6 g of Sodium hydroxide (NaOH) in 250 g of…

A:

Q: a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of…

A: Electrolyte is a material which if dissolved into a polar solvent, generates an electrically…

Q: An electrochemical cell is based on the following two half-reactions: oxidation: Sn (s) →Sn²+ (aq,…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2MNO,…

A: Given-> [MnO4-] = 3.06 M [H+] = 1.02 M [Mn2+] = 4.19 M [Pb2+] = 2.07M

Q: 11.)

A: We have given that From representation of the cell reaction  Oxidation half reaction :  Zn(s)…

Q: 3.13 The oxidation of ferrous iron (Fe²+) to ferric iron (Fe) by molecular oxygen can be described…

A: The standard free energy of formation of Fe2+ (aq) is -75.0 kJ/mol, the standard free energy of…

Q: Reduction Half-reaction Half-cell E (V) Oxidizing Agent F(g) + 2e HO, (aq) + 2 H*(aq) + 2 e" PhOs) +…

A: Given that, the standard reduction potential table. (1) We have to tell if Al(s) is able to reduce…

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

A: The answer is as follows:

Q: Calculate the standard reaction free energy delta G for the following redox reaction. Round to 3…

A:

Q: Write the balanced net ionic equation for the reaction of aqueous sodium sulfate with aqueous…

A: Steps followed while writing the balanced net ionic equation : 1): write balanced moleculer…

Q: Give only typing answer with explanation and conclusion to all parts 1. (a)Given the following…

A: (a) To calculate the solubility product of AgCN at 25°C, we need to use the Nernst equation and the…

Q: aq), I2 (g), and I (aq), the strongest

A: 1) Strongest Oxidising agent : Those species which is easily reduced by gaining of electrons.  2)…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a.)

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

A: The solution is as follows:

Q: 14.58 Complete and balance the following oxidation-reduction reactions, assuming they occur in…

A: Here we are required to balance the redox reaction.

Q: ) For the concentration cell: Pt(s) | H2(g), H+(aq) (pH = 10) || H+(aq) (pH = 4), H2(g) | Pt(s),…

A: From nernst equation, E cell can be calculated

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A:

Q: What mass of Ba(s) may be deposited from an aqueous BaCl2 solution if a current of 2.50 A is applied…

A: Mass of electrodeposited species can be calculated from the amount of charge passed.

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

A:

Q: The following reaction occurs in an electrochemical cell: 3 HCIO,(aq) + 2 Cr³* (aq) + 12 H2O(e) → 3…

A: Given: The concentration of Cr2O72-, HClO2, and [HClO] is 0.80 M, 0.15 M and 0.20 M, respectively.…

Q: (c) the solution that results from mixing 25.0 mL of 0.0500 M KBr with 20.0 mL of 0.100 M Ag*.…

A: Electrode potential is the potential of the cell that consists of an electrode acting as cathode and…

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V  PH2=0.857atm Concentration of Cd2+=1.00M

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: An

A: We will calculate nfactor

Q: Consider the following half-reactions: Half-reaction E° (V) 2(s) + 2e 21°(aq) 0.535V Ni2+ "(aq) +…

A: We are given the standard reduction potentials of different half cell reactions. We must know that…

Q: Given the following standard electrode potentals: Ag°(aq) + e¯ = Ag(s) N,(g) + 5H°(aq) + 4e° =…

A: Consider the given values as; Ag+ aq + e- ⇌ Ag s…

Q: (a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing…

A: Note- Since you have asked multiple questions, we will solve the first question for you. If you want…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

A:

Q: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

A: An aqueous sodium chloride solution is electrolyzed using a current of 4.42 A. How much time (min)…

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.