What quantity of electric current is required to deposit 0.750 g of Pt(s) from a solution containing the [PtCl4]2– ion within a time of 2.50 hours?

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

A: Given,The redox reaction:ClO3- (aq) + C2O42- (aq)  ClO2 (g) + CO2 (g)

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Q: Balance the following equations and identify the oxidizing and reducing agents a. NO, (ag) + Cr,0,2…

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Q: In acidic conditions, manganate(VII) ions are reduced to manganese(II) ions, Mn. In neutral…

A: The balanced equations for the reduction of manganate(VII), MnO4-(aq) in acidic and neutral medium…

Q: 11. Balance the following Redox reaction that takes place in basic solution. Identify the oxidizing…

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Q: 9. Predict whether Co2* can oxidize Cl to Cl2 under standard state conditions. Explain your answer…

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Q: Balance the following oxidation–reduction reaction in basic solution. MnO4 –(aq) + I–(aq) -->…

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Q: Complete and balance the following redox reaction in acidic solution. Cr2O,2-(aq) + Pb²*(aq) →…

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Q: Metal Metal ion Pb²+ (aq) Re³+ (aq) In³+ (aq) TI¹*(aq) Pb(s) Re(s) In(s) TI(S) Pb(s) Re(s) In(s)…

A: An oxidizing agent is that species which accepts electrons makes oxidize another species. The agent…

Q: Classify each half-reaction as a reduction or an oxidation. oxidation Cr,0 (aq) + 14 H' (aq) + 6 e 2…

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A: The given unbalanced equation is, CrO72-(aq)+C2H5OH(aq)→Cr3+(aq)+CO2(g) First we need to balance…

Q: 4. Write balanced equations for the following reactions in basic solution. (a) SO2(g)+I2(aq)→SO3(g)+…

A: Since you have asked a question with multiple subparts we will answer the first three for you. To…

Q: Four metals (A, B, C, and D) were studied for activity, and the following information was  collected…

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Q: Complete and balance the following redox reaction in basic solution Pb2-(aq) + 10:-(aq) → PbO:(s) +…

A: In basic media, OH− ions and water are added to half reactions to balance the overall reaction.  The…

Q: If a redox reaction occured with the 2 redox couples provided below, which species would be the…

A: The species which has greater reduction potential that tends to reduce itself and oxidize other…

Q: Which of the following metals is most likely to become oxidized (act as O Ca2+(aq)+2e¯→ Ca(s) E°red=…

A: Introduction : Oxidation means loss of electron .

Q: Balance the following reaction in basic solution. Ag(s) + Zn²+ (aq) → Ag₂O(aq) + Zn(s) Fill in the…

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Q: What quantity of electric current is required to deposit 0.750 g of Pt(s) from a solution containing…

A: Here, The amount of Pt(s) deposited from [PtCl4]2- ion solution = 0.750g. Time required for…

Q: When the following skeletal equation is balanced under acidic conditions, what are the coefficients…

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Q: Consider the reaction: - Fe(OH),(8) + Pb(OH), (aq) → Fe(OH),(8) + Pb(s) [basic]| Which atom is being…

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Q: An acidic solution of permanganate (MnO4–) ions can oxidize nitrous acid to nitrate ions. The…

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Q: Balance the reaction below in basic solution. • identify the species oxidized, the species reduced,…

A: The given unbalanced redox reaction, MnO4− (aq) + Br− (aq) → BrO3− (aq) + MnO2 (s)

Q: A total of 1.558 F of electricity (1 F = 1 mol e) was required to electrodeposit all of the Zn and…

A: ZnSO4 and CoSO4 both have divalent metal ions as, Zn2+ and Co2+.   (Here M= metal)So, 2F electricity…

Q: Complete and balance the following redox reaction in acidic solution. Be sure to include the proper…

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Q: Balance the following redox reaction in acidic solution. 3+ NO(g) + Fe³+ (aq) 2+ HNO₂(aq) + Fe²+…

A: Unbalanced reaction : NO (g) + Fe3+(aq) →HNO2(aq) + Fe2+(aq)

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Q: Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C…

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Q: 14. Balance the following reaction in basic solution Fe(OH)2(s) + MnO4 (aq) → MnO2 (s) + Fe(OH)3(s)

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Q: For a particular redox reaction, NO₂ is oxidized to NO3 and Fe³+ is reduced to Fe²+. Complete and…

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Q: Identify the oxidizing and reducing agents in the skeletal (unbalanced) reaction. Then, balance the…

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Q: can cadmium metal (Cd(s)) reduce cobalt (II) ions (Co2+(aq)) to cobalt metal

A: cadmium can only reduce cobalt if its reduction potential is smaller than that of cobalt.

Q: Balance the following redox reactions that occur under acidic conditions.   2. MnO4-1 (aq) +   H2O2…

A: we have to balance the given redox reactions in acidic solution

Q: 5. Consider the following half-reactions: F,(g) + 2 e Cu2*(aq) + 2 e Sn2*(aq) + 2 e → AР' (aq) + 3 e…

A: Which of the above elements or ions will oxidize Sn(s)?

Q: Write balanced half-reactions for the following redox reaction: 5 Ch(9)+2 Mn (aq)+16 OH (aq) → 10 CI…

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Q: Complete and balance the following redox reaction in acidic solution IO3^-(aq) + ClO2^-(aq) ->…

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Q: Balance the following net ionic equation for a redox reaction in acidic solution. Mg(s)+ NO3–(aq)…

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Q: For a particular redox reaction, NO₂ is oxidized to NO3 and Cu²+ is reduced to Cut. Complete and…

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Q: Cu+ (aq) + Cu(s) K = 6.2 × 108 2+ Pb²+ (aq) + 2e¯ = Pb(s) K = 4.0 × 10-5 Fe³+ (aq) + 3e = Fe(s) K =…

A: Higher the value of reduction potential or equilibrium constant, higher is the tendency of 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.