Select the correct species to complete the sentences below. a) Cr3+(aq) + 3e- → Cr(s) Eº = -0.73 V Mn2+(aq) + 2e- → Mn(s) Eº = -1.18 V What species will spontaneously reduce what species? b) ClO2(g) + e- → ClO2-(aq) Eº = 0.95 V Sn4+(aq) + 2e- → Sn2+(aq) Eº = 0.15 V What species will spontaneously oxidize what species?

Q: Complete and balance the following half-reaction in basic solution 2- Cr(OH)3(s) → CrO4²- (aq)

A: A redox reaction is balanced by balancing the mass and charge. Hence the number of atoms of all the…

Q: The following standard reduction potentials have been determined for the aqueous chemistry of…

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Q: Consider the following half-reactions: Cl2(9) + 2e - 2cF (ag) = 1. %3D I2(9) + 2e - → 21 (aq) E, =…

A: From given data ,  based on the E° value given for the half actions we can predict the strongest…

Q: the substances.             [PtCl4]2–(aq) + 2 e–  ⟶⟶ Pt(s) + 4 Cl–(aq); E° = 0.755 V…

A: The answer is given as follows

Q: 31. Given the standard reduction potential (E0) values below, calculate the equilibrium constant…

A: Each Electrochemical reaction can be described by a cell potential value that varies with the chosen…

Q: Use the oxidation method to balance the following reactions. a) IO3- (aq) + HSO3- (aq) SO42- (aq) +…

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Q: Consider the following reductions. Cu+(aq) +  e- ⟶⟶ Cu(s)                                     Eored…

A: Oxidizing agent:-  It is a substance that oxidizes other substances and gets reduced by itself.…

Q: Select the best oxidizing agent based on the standard reduction potential for the species shown. O…

A: In the electrochemical cell, the chemical energy is converted into electrical energy.The addition of…

Q: Consider the following half reaction NO3(aq) + 10 H+ (aq) + 8e -> NH4+ (aq) + 3H₂O(1) If the ratio…

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Q: Complete and balance the following redox reaction in basic solution Cr20,2-(aq) + Hg(1) → Hg²"(aq) +…

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Q: Consider the following two half-reactions and their standard reduction potentials, and answer the…

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Q: Complete and balance the following half-reaction in acidic solution N,(g) → NH,*(aq)

A: N2(g) = NH4^+(aq)  Or, N2(g) = 2NH4^+(aq) (N atom balanced) Or, N2(g) + 8H^+(aq) = 2NH4^+(aq) (H…

Q: 3Ce+ (aq) + Bi(s)+ H2O(1)→3Ce3+ (aq) + BiO+ (aq)+2H+(aq) Express the equilibrium constant to two…

A: Given,  Part. B :-  Balanced reaction is :  3Ce4+ (aq) + Bi (s) + H2O (l) ------> 3Ce3+ (aq) +…

Q: Complete the stepwise process of balancing the following reaction in acidic conditions. Cr20;²"(aq)…

A: The unbalanced equation is  Cr2O7–2 (aq)  + HNO2 (aq) -------> Cr+3 (aq) + NO3– (aq) In this…

Q: onsider the following equilibrium system:  MnO4− + 4 H+ + 3 e− ⇌ MnO2(s) + 2 H2O(l) (a) Calculate…

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Q: Calculate the equilibrium constant of the reaction 2 Ti2+ + Sn4+ ↔ 2 Ti3+ + Sn2+ Sn4+ + 2e- ↔ Sn2+…

A: Ecell°=ESn4+/Sn2+° - ETi3+/Ti2+°      = 0.154 --0.369      = 0.154 + 0.369      = 0.523 V Formula:…

Q: Discuss the spontaneity of an electrolytical reaction in terms of its standard emf (Eocell)If a…

A: Spontaneous reaction can be defined as the reaction that occur by itself without any external source…

Q: Calculate the equilibrium constant for each of the reactions at 25 oC. Br2(1 )+2CI-(aq) ->…

A: The subsequent solution involves algebraic manipulation and, if provided, the utilization of…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) +…

A: The given cell reaction is, 2Ag+(aq) + H2(g) → 2Ag(s) + 2H+(aq) To find: The equilibrium constant?…

Q: 1. Given the electrochemical reaction shown, what is the standard free energy of change if E* =…

A: The electrical work done in a galvanic cell is the product of the electricity (charge = nF) passed…

Q: a. Under standard-state condițions, which is the strongest oxidizing agent? [ Select ] b. Under…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Based on the following electrochemical data, which is the strongest oxidizing agen Hg2+(aq) + 2e →…

A: Oxidizing agent :  If the reduction potential of a species is high or more positive then it will…

Q: Given the following standard reduction potentials: MnO4 (aq) + 8H*(aq) + 5 e - - Mn2*(aq) + 4 H20()…

A: The expression of Nernst equation is shown below: E =E0cell -0.0591n log Q Where; Ecell= cell…

Q: Co³*(aq) + e¯ → Co²*(aq) → Fe²+(aq) E° = +1.953 V Fe*(aq) + e¯ E° = +0.769 V %3D I;(aq) + 2e¯ –→…

A: Since we only answer up to 3 sub parts, we'll answer the first 3. Please resubmit the question and…

Q: 13.40 Calculate the equilibrium constant for the following reac- tions using data from the standard…

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Q: The voltaic cell Ca(o)Ca²+ (aq) || Ni?+(1.0 M)|Ni(s) has a cell potential of 0.300 V at 25°C. What…

A: Given : Ecell = 0.300 V Temperature = 25 oC Concentration of Ni2+, [Ni2+ ] = 1.0 M And Eocell =…

Q: Given the redox reaction: MnO4- + Fe2+ → Mn2+ + Fe3+   Calculate the oxidation state for Mn in the…

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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.