How many amperes are required to deposit 0.180 grams of lead metal in 670. seconds, from a solution that contains Pb2+ ions .

Q: Which of the following metals will be oxidized by Pb1NO322: Zn, Cu, Fe?

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Q: Calculate the charge, in coulombs, is required to deposit 1.5 g of solid magnesium from a solution…

A: The answer to the following question is- Given, mass of magnesium = 1.5 g  Molar mass of magnesium =…

Q: sample of iron ore weighing 0.2732 g was dissolved in an excess of a dilute acid solution. All the…

A: Given sample of iron ore weighing 0.2732 g  24.70 mL of 0.0174 M KMnO4 for oxidation to Fe(III) ions…

Q: How many amperes are required to deposit 0.256 grams of manganese metal in 380. seconds, from a…

A: The reaction occurring will be  Mg2+ + 2 e-  ----> Mg (s) Hence the number of electrons required…

Q: How many grams of nickel remains in a 100 ml of 1.50 M NİCI4 solution if 3.0 ampere current is…

A: V = 100 ml = 0.1 L M = 1.50 M I = 3 Amp t = 1 hr = 60 x 60 = 3600 sec W = ? nf = 4 By using Faraday…

Q: Balance the following electrochemical reaction in acid: MnO 4 (aq) + Zr( s) → Mn –"( aq) + Zr + Zr…

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Q: What is the value of the equilibrium constant for the reaction between each pair at 25°C? (a) Ni(s)…

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Q: How many amperes are required to deposit 0.106 grams of tin metal in 333 seconds, from a solution…

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Q: Name the method of refining of the following metals – (a) Hg (b) Sn (c) Cu (d) Ge (e) Ni (f) Zr

A: a) Hg = The method used for the refining of the given metal is Distillation.       b) Sn = The…

Q: How many amperes are required to deposit 0.119 grams of nickel metal in 806 seconds, from a solution…

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Q: gallium (s) | 0.025 M gallium sulfate (aq) | 5 M KNO3 | 0.025 M copper (II) fluoride (aq) | copper…

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Q: If 612 C of charge is passed through a solution of Cu(NO3)2(aq), calculate the number of moles of…

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: Balance the following reaction in acidic solution. Cr20 (ag) + HNO2(aq) → Cr**(aq) + NO, (ag) Cr3+

A: Balancing the chemical equation involves many steps. There is a difference in the balancing of the…

Q: Complete and balance the reaction in acidic solution. equation: ZnS + NO, Zn²+ + S + NO Which…

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Q: Write balanced equations for the following redox reactions: a. 2 NaBr + Cl2 2 NaCl + Br2 b. Fe2O3…

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Q: How many grams of cobalt may be formed by the passage of 3.71 amps for 2.68 hours through an…

A: According to the Faraday's first law of electrolysis, the amount of chemical change which will take…

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: + IO3 (ag) I, (agi (Acidic)

A: The reaction given is, => I- (aq) + IO3- (aq) -------> I3- (aq) In the above reaction, I is in…

Q: Complete and balance the equation for the single displacement reaction between lithium and cadmium…

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Q: What is the redox reaction of hypochlorite if titrated with sodium thiosulfate?

A: Redox reaction: It is a kind of reaction in which one species is oxidized and while the other is…

Q: The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the…

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Q: How to balance this redox reaction? KMnO4 + FeSO4 + H2SO4 → K2SO4 + Mn+2SO4 + Fe2(SO4)3+ H2O

A: The number of electrons lost during the oxidation is equal to the number of electrons gained during…

Q: Complete and balance the following redox reaction in basic solution. ReO, (aq) + Pb²*(aq) → Re(s) +…

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Q: When the following redox equation is balanced under acidic conditions with the smallest whole-number…

A: Cr3+(aq) +Cr(s) →Cr2+(aq)Reduction half reactionCr3+(aq) →Cr2+(aq)On LHS total positive charge =…

Q: Identify the oxidation numbers to all the elements in each of the compound or ior Na O a. Na=3 Ob.…

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Q: 4. Write balanced equations for the following redox reactions: a. NaBr + Cl2 → NaCl+Br2 b. Fe:Os +…

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Q: Which of the following metals will react with HCl to form hydrogen gas? A. Hg B. Au C. Cu D. Ag…

A: The following metals will react with HCl to form hydrogen gas has to be given,

Q: What charge, in coulombs, is required to deposit 0.205 g Ag(s) from a solution of Ag *(aq)? О а. 197…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: How many grams of copper nitrate (Cu(NO3)2) should be added into 1000 ml water to produce a half…

A: Given data,Volume of water=1000mLElectric potential=0.32VNernst equation;E=Eo-0.0591nlogQ   ---at…

Q: 4. Assign oxidation numbers to all elements in the following, balance the equation and calculate the…

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Q: Write balanced equations for the following redox reaction: Cu + HNO, - Cu(NO3)2 + NO + H,O (in…

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Q: How many amperes are required to deposit 0.146 grams of chromium metal in 678 seconds, from a…

A: Given: mass of chromium metal = 0.146 g time = 678 seconds charge = 3 molar mass of Cr = 52 g/mol

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

A: Balanced the half reaction under given condition in the question.

Q: Complete and balance the following reaction, then give the product side of the balanced equation.…

A: In given reaction zinc oxidised and iron reduced

Q: For the following redox reaction, calculate E0cell, ∆G0rxn and the equilibrium constant, K. The…

A: From the reaction: Reduction Half Reaction is- Here, MnO2 is reduced (Cathode) and its…

Q: Complete and balance the reaction in acidic solution. equation: ZnS + NO, Zn2+ +S + NO > Which…

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Q: one of the following metals is used as oxidizing agent a. Ca b. Na c. Fe+2 d. Fe+3

A: Oxidising agent :- The oxidizing agents are those species which can oxidise other species and can…

Q: Explain why chlorine gas can be prepared by electrolyzing an aqueous solution of NaCl but fluorine…

A: We wil write the required explanation

Q: Complete and balance the reaction in acidic solution. equation: ZnS + NO3 Zn²+ +S + NO

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Q: How many amperes are required to deposit 0.219 grams of zinc metal in 710. seconds, from a solution…

A: According to the first law of Faraday, the mass of a metal deposited on the cathode during…

Q: 2.284 g of tin was oxidized through the titration. What is the mass percent of tin in the original…

A: Given-> Weight of tin(Sn) = 2.284 gm Weight of ore sample = 10.00 gm

Q: Which metal would be suitable for use as a sacrificial anode for iron? O Au O Mg Cu Pt Sn

A: Sacrificial anode - In this technique, the metal to be protected is made cathode and is connected to…

Q: Determine the Oxidation Numbers of each element in the following substances: a. Li,o Li: 0: b. Cr,0,…

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

Q: Complete and balance the following redox reaction in basic solution 10s (aq) → Iz(s)

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Q: How many coulombs will it take to deposit 8.97 g of metallic copper on the cathode from an aqueous…

A: The metal will be reduced at cathode as follows: Cu2+(aq)  +  2e-  ------------->  Cu(s).

Q: Complete and balance the following half-reactions. In each case, indicate whether the half-reaction…

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

Q: When 1.00 mole of chlorine gas is reduced to chloride ions in an electrolytic cell, what charge (in…

A: Reduction of 1 mol of chlorine is given below, Number of moles of electrons is 2.

Q: 17) The number of Faraday of charge needed to deposit 3.54 x 10-4 moles of Cr+3 ion from its…

A: In this question, we want to determine the number of Faraday of charge.  Given : moles of Cr3+ ion…

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.