Complete the following redox problems: a. Write the balanced equation and find the value of E for the reaction made from the half reactions: 2 CLO3-(aq)+12 H+(aq) + 10 e-  --> Cl2(g)+ 6 H2O(l)       E0= 1.47V NO3-(aq) + 4 H+(aq) + 3 e- --> NO(g) + 2 H2O(l)     E0=0.96V   b. What are the half-reactions for the reaction: 2 Al(NO3)3(aq) + 3 Zn(s) --> 2 Al(s) + 3 Zn(NO3)2(aq)

Q: Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in…

A: The redox reaction balancing in acidic medium -  Oxygen is balanced by addition of water Hydrogen…

Q: 3. Rosenberg was studying the electric field effect on bacterial growth when he unknowingly carried…

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Q: A redox reaction has E°cell = +0.88V. What can you conclude about ΔG° and K for this reaction?…

A: Given:  E°cell = +0.88V To find: i) ΔG°   ii) K

Q: How many electrons were gained by vanadium in the given half-reaction? vo,- → v- а. 1 с. 3 b. 2 d. 5

A: Balance the given half-reaction in order to determine the number of electrons gained by vanadium.

Q: Given a redox reaction: 3S(k) + 2KClO3 (k) 3SO2 (g) + 2KCl (k) a) Identify and underline the element…

A: # In oxidation, oxidation number of element increases.    # In reduction, oxidation number of…

Q: FORLAD 4 Consider the redox reaction where Ag+ (aq) is oxidized to Ago (s) (E° 0x = -1.77 v) and…

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Q: 20.51 Given the following reduction half-reactions: Fe (aq) + e Fe2 (aq) Eed = +0.77 V S,02 (aq) +…

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Q: 1. Using the half reactions shown below, determine the balanced net reaction, E° for the net…

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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: The balanced half-reaction occuring at the cathode in the redox reaction shown below is 3MnoAlao)…

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Q: ow many grams of Ag(s) (107.9 g/mol) could be plated out on the cathode of an electrolytic cell by…

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Q: A voltaic cell consists of a copper electrode in a solution of copper (II) ions and a palladium…

A: Estimation of electrodes' potential difference used in any cell is recognized by the term "cell…

Q: Write the half reaction in the cathode, if the Copper + cation is reduce to form cupper metal.…

A: Given data : Copper + cation is reduce to form cupper metal. Find out : half cell reaction in the…

Q: 20.72 A voltaic cell is constructed that is based on the following reaction: Sn²* (aq) + Pb(s) Sn(s)…

A: A voltaic cell is constructed based on the following reaction: Sn2+(aq)+Pb(s) → Pb2+(aq)+Sn(s)

Q: Consider the following half-reaction containing acid HX below.   3 N2(g) + 2 H+(aq) + 2 e-  →  2 HX…

A: given:  O3(g) + 2 H+(aq) + 2 e-  →  O2(g) + H2O (l)  E°red = 2.076 V   find: Could HX be applied to…

Q: Calculate AGn and Ee for a redox reaction with n = 2 that has an equilibrium constant of K = 25 (at…

A: Given data Equilibrium constant : K=25    at temperature T=25 °C=(25+273) K = 298 K Number of…

Q: Semimetallic silicon can be made by the electrolysis of molten SiO2. (a) What mass of Si is formed…

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Q: Given the following reduction half-reactions: Fe+ (aq) + e": S2O6² (aq) + 4H* (aq) + 2e¯ → 2 H2SO3…

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Q: The balanced half-reaction occuring at the cathode in the redox reaction shown below is + 5Fes) +…

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Q: Calculate the equilibrium constant at 35°C, for the redox reaction between Au (aq) and Br(aq). HINT:…

A: Given reduction half-reactions with E0 values:

Q: Balance the following half-equations and hence determine an overall equation for the reaction of…

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Q: What mass of Iron, Fe, will be produced in a cell using Fe(NO3)3 if a current of 5.0A is maintained…

A: Given, Current flow = 5 A, Time = 2 hours = (2 * 3600)…

Q: 2. 1) Given the following battery: Au*/Au° and Ni*2/Ni° calculate Eo. 2) If you wanted to improve…

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Q: (Q91) What is the value of the equilibrium constant (Keq) when the following reaction occurs at…

A: Answer: 4th option : 5.5* 10^30

Q: How many grams of nickel (58.69 g/mol) may be electroplated by passing a constant current of 7.2 A…

A: Total charged apssed = current ×time in seconds.=7.2×34×60= 14688 columb . Ni is formed through the…

Q: How many grams of X (MW = 157.49 g/mol)(in g) will be deposited on a cathode in 2.11 h by a current…

A: Faradays First Electrolysis Law provides that the amount of reaction taking place on the basis of…

Q: Q5. Chlorine is an important industrial chemical. (a) Chlorine is formed when KMNO, reacts with…

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Q: 2) The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing…

A: Options  D) The oxidation of half reaction ,     Fe2+ (aq)  → Fe3+ (aq) + 1e- The Reduction of half…

Q: For the following electron-transfer reaction: 3Zn?+ *(aq) + 2Al(s) –→ 3Zn(s) + 2A1³* *(aq) The…

A: Observing the given reaction shows that it contains both oxidation and reduction reaction. Loss of…

Q: 0 (@) what is 16° for the reaction O > Cu + + Fe3+ fe 2+ Cu²+ + Fe²+ Use the following potentials:…

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Q: Of the following, which one is most likely to be the strongest reducing agent: O2, 02", 02 ?O22…

A: Strong reducing agent is O2+. Correct option is A.

Q: Balance redox reactions using the half-reaction method. Balance the redox reaction below using the…

A: The reaction given is, => Ir3+ (aq) + Hg (l) → Ir (s) + Hg22+ (aq)

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: In a electrolytic process, cations go to the anode and anions go to the cathode.

Q: The balanced half-reaction occuring at the cathode in the redox reaction shown below is 3MnOlag) a)…

A: Answer: Reduction always takes place at cathode and oxidation always takes place at anode.   In the…

Q: Balance the following redox reaction under basic aqueous conditions using the smallest whole-number…

A: The given reaction is balanced as follows,

Q: 1. The following redox reaction was constructed at 25.0°C. Pb²+ (aq) + Mg(s) → Pb(s) + Mg²+ (aq) a.…

A: The redox reaction at 25.0°C  :  Pb2+(aq) + Mg(s) ---> Pb(s) + Mg2+(aq)  a) Half reaction occurs…

Q: 6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H (aq) +2 e → 2 HX…

A: Solution: A) Yes, we can see the standard reduction potential is - 3.09 V. Since we know standard…

Q: (1) An electrochemical cell contains an SCE anode and a lead cathode. The solution around the lead…

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Q: 3. Rosenberg was studying the electric field effect on bacterial growth when he unknowingly carried…

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Q: Half Reaction A: 2H+ + 2e- ---> H2 (at standard conditions, pH 0 ) Half Reaction B: S + 2H+ + 2e-…

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Q: 6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H* (aq) +2 e → 2 HX…

A: We know that,      Gibbs free energy, ∆G° = -nFE°  Where, n is the no. of electrons oxidize or…

Q: In a process of electroplating silver, a current of 15.2 amps (A) was passed through an electrolytic…

A: Since you have posted multiple questions, we are solving the first question. Please post rest of the…

Q: Number 1

A: A reduction reaction involves gain of electron/s. Due to gaining of electron/s, the oxidation number…

Q: (a) In the electrolysis of aqueous Naz2C204, how many liters of H2(9) (at STP) are generated by a…

A: The balanced chemical reaction can be written as follows: Na2C2O4 (aq) +  2H2O (l)  →  2CO2 (g) + H2…

Q: Write two half-equations for the following sreactions. For each half-equation state whether…

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Q: ow many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of…

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Q: 8. For the oxidation-reduction reaction: S406(aq) + Cr+(aq) Cr (aq) + S202 (aq), -> the appropriate…

A: recall the given half cell reactions Reduction half cell reaction     S4O62-+2e-→2S2O32-  ......(i)…

Q: What are E°cell and ΔG° of a redox reaction at 25°C for which n=2 and K=65?

A: Under standard reaction condition is known the potential of the cell is known as the cell potential.

Q: How many grams of X (MW = 91.45 g/mol)(in g) will be deposited on a cathode in 1.15 h by a current…

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Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A: The reaction considered is, Cr2O7+ (aq) + 14H+ (aq) + 12 e-→12 Cr (s) + 7 H2O

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.