complete and blance the following oxidation-reduction reactions, which give the highest possibleoxidation state for the oxidized atoms. (a) K(s)+H20(l)  (b) Ba(s)+HBr(aq) (c) Sn(s)+12(s)

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: Calculate the equilibrium constant (KP) for the following reaction at 25°C:

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Q: 6. If the cell potential in the previous problem (5) is 0.485 V, what is the [CI] in the cathode…

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Q: In the electrolytic refining of copper,what factor determines which piece of copper is theanode and…

A: In the electrolytic refining of copper, what factor determines which piece of copper is the anode…

Q: What feature of an oxidation-reduction reaction allowsit to be used to generate an electric current?

A: What feature of an oxidation-reduction reaction allowsit to be used to generate an electric current?

Q: (a) Consider the following equation NO:(g) + H:0(1) – HNO:(aq) + NO(g) (i) Write two balanced…

A:

Q: 5. The mass of metal deposited by the electrolysis of an aqueous solution of metal ions increases in…

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Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

A:

Q: Balance the net ionic redox equations by the half-reaction method: full reaction balanced in acid:…

A: In order to balance a net ionic equation by the half-reaction method, we separate both the…

Q: * Complete and balance the following redox reaction in acidic solution AIO2 (aq) + PO3" (aq) → Al(s)…

A: The given reaction is AlO2- (aq) + PO33- (aq) → PO43- (aq) + Al (s).

Q: 19.95 In the commercial preparation of aluminum, alu- minum oxide, Al,O3, is electrolyzed at 1000°C.…

A: Given: Mass of Al = 3.09 Kg = 3090 g Reaction at cathode:  Al+3 + 3e- → 3Al

Q: A solution of silver nitrate containing 12.14 g of silver in 50 ml of soluti on was electrolysed…

A: Initial mass of Ag in silver nitrate = 12.14 g Volume of solution = 50 ml After electrolysis, mass…

Q: The cathode reaction is: AUA13+

A: The voltaic cell is basically an electrochemical cell that generates electrical energy using a…

Q: Consider the following redox reaction with nitrogen (N): NO3 + H* + 8e +→ _NH4* a. Balance this…

A:

Q: Complete and balance the following redox reaction in basic solution CIO:(g) → CIO2 (aq) + CIO3 (aq)

A:

Q: Complete and balance the following redox reaction in basic solution CIO2(g) → CIO2 (aq) + CIO3 (aq)

A: 2 ClO2 + 2 OH- → ClO2- + ClO3- + H2O

Q: Complete and balance the following redox reaction in acidic solution 10, (aq) + CIO2 (aq) → 12(s) +…

A:

Q: Complete and balance the following redox reaction in acidic solution   As(s) --> H2AsO4- (aq) +

A: The question is based on the concept of redox reaction. we have to balance the given equation.

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: Balance the following redox reactions: (a) In acidic solution, xenon trioxide reacts with iodide ion…

A: Since you have posted multiple sub-parts, we will solve the first three sub-parts for you. To get…

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

A:

Q: What is the chemical reaction for the electrolysis of Cu/H2SO4 electrolyte? Provide the enthalpy of…

A: Chemical reaction for the electrolysis of Cu/H2SO4 electrolyte Enthalpy of the reaction.

Q: Complete and balance the following redox reaction in basic solution 10, (aq) + Re(s)→ ReO, (aq) + 1O…

A: (9)

Q: Complete and balance the following redox reaction in basic solutio Zn(s) → Zn(OH),²(aq) + H,(g)

A: A chemical reaction is the representation of reactants and products along with their chemical…

Q: In the commercial preparation of aluminum, aluminum oxide, Al2O3, is electrolyzed at 1000°C. (The…

A: Given- mass of aluminum = 3.09 kg Reaction Al3+ + 3e- ----> Al To find- coulombs of electricity…

Q: Explain the Stoichiometry of Electrolysis?

A: The weights of substances formed at an electrode during electrolysis are directly proportional to…

Q: How many grams of silver metal are produced from Ag*(aq) in 4.05 h with a current of 3.50 A? (F =…

A:

Q: Example:- Calculate the normality of a solution of 0.25 gm/L H2C¿O4, both as an acid and as a…

A: Normality of the solution is given by the number of gram equivalents per litre of the solution.

Q: In an electrolysis experiment, a student passes the same quantity of electricity through two…

A:

Q: Predict the products and balance the following eqn. and identify the type of reaction FeCl. 3(aq) +…

A:

Q: C. Calculate the concentration of the Zn²+(aq) ion at the cathode.

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Q: A current of 3.27 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

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Q: Nitrate ion substitutes for oxygen as an electron acceptor in the biodegradation of organic matter,…

A: Ideal gas equation is given by: PV=nRT      OR PV=mMRT         .....(1) Where, 'P' is the pressure,…

Q: Commercial aluminum production is done by the electrol-ysis of a bath containing Al₂O₃ dissolved in…

A: The commercial production of aluminum is achieved by electrolysis of bath that contains Al₂O₃…

Q: How many moles of Al3+ would be electrolyzed to Al(s) with the same amount of electricity that…

A: According to Faraday law of electrolysis - The amount of substance deposited at electrode is…

Q: Cu(NO,), would you expect

A: We can write the balanced equation and can determine the theoretical yield from the equation.  The…

Q: What is the half reaction corresponding to the conversion of FeO42- to Fe(OH)3?

A: In the conversion of  FeO42- to Fe(OH)3 the Fe ion is basically converting from 6+ to 3+ state.…

Q: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If…

A:

Q: A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is…

A: Atomic Mass of Br - 79.904 u Atomic Mass of Cl - 35.5 u Molar mass of AgCl - 143.32 g/mol Molar mass…

Q: 17. When metallic lithium is a reactant in a synthesis reaction with oxygen gas to form an ionic…

A: The balanced equation for reaction between metallic lithium and oxygen gas is ...    4Li     +   O2…

Q: Balance the following redox reaction in acid: MnO4 – (aq) + C2O4 2– (aq) → Mn2+ (aq) + CO2 (g) a.…

A:

Q: At 18°C a 0.001-M aqueous solution of potassium hydrogen carbonate, KHCO3 , conducts a current in a…

A: Potassium bicarbonate dissolve in water. It dissociate into water to produce potassium ion ( K+)…

Q: I know the answer needs to be positive, but I keep getting a negative. Why?

A:

Q: 2. Which of the metal(s) Ni , Ca, K, Fe, Ag, will not react in an aqueous solution of Al(NO,); to…

A: generally more  metals react with metal salts to displace the metal present in the metal salt  it is…

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

A:

Q: Complete and balance the following redox reaction in acidic solution Teo, (aq) + N,O̟(g)→ Te(s) +…

A: The given redox reaction is: TeO32-aq+N2O4g→Tes+NO3-aq

Q: How are atomic size, IE₁, and EN related to redox behaviorof the elements in Groups 1A(1), 2A(2),…

A: Atomic Radius -It is the distance between the nucleus of the atom to the last electron containing…

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.

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.