Complete and balance the following redox reaction in acidic solution:  AlO2- (aq) + PO33- (aq) --> Al (s) + PO43- (aq)

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

Q: Complete and balance the following redox reaction in basic solution Zn(OH),2- (aq) + As (s) → Zn(s)…

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Q: What volumes of H2 (g) and O2 (g) at STP are produced from the electrolysis of water by a current of…

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Q: During a period of discharge of a lead–acid battery, 402 gof Pb from the anode is converted into…

A: Overall cell reaction is Pb(s) + PbO2(s) + 2H+ (aq) + 2HSO4- → 2 PbSO4 + 2H2O Where, 1 mol of Pb is…

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

A: The chemical reaction corresponding to electroplating of Chromium is given as:Cr2O72- (aq) + 14 H+…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

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Q: For the cell shown, the measured cell potential, ?cell, is −0.3681 V at 25 °C.   Pt(s) |…

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

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Q: How many grams of Au would be deposited from an aqueous solution of Au 3+ with a current of 2.213 A…

A: Given, Molecular mass of Au = 196.96 u Current = 2.213 A time = 480 minutes = 28,800 sec

Q: What mass of Cu(s) Cu(s)is electroplated by running 12.5 A Aof current through a Cu 2+ (aq)…

A: Given: T= 4*60*60 =14400 sec Current= 12.5 A

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

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

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

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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: Rank the halogens by oxidizing strength and the halide ions by reducing strength from strongest to…

A: A question based on redox reaction, which is to be accomplished.

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: How many minutes will it take to electroplate 42.1 g of gold by running 5.00 A of current through a…

A: In an electrolytic cell for the electrolysis of a metal conversion of electrical energy in to…

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

A: The given equation is, 2NO3-+12H++10e-→N2+6H2O Pressure = 1.00 atm. Temperature = 298 K. Molar mass…

Q: Predict whether the following reactions will be spontaneousin acidic solution under standard…

A: When Gibb's free energy of a reaction delta G is negative, then the reaction is spontaneous. When…

Q: Balance the following reactions in both acidic and basic media, identify the oxidation and reduction…

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Q: Complete and balance the following redox reaction in acidic solution H2O2(aq) + Cr2O,2-(aq) → O2(g)…

A: Redox reactions are those in which one of the molecules is reduced and the other gets oxidized. The…

Q: Ozone (O3) and chlorine dioxide (ClO2) are both strong oxidizing agents. Given the half reactions…

A: Given half cell reactions are : O3 + 2H+ + 2e- = O2 + H2O, E0 = 2.07 V vs. SHE ClO2 + e- = ClO2-, E0…

Q: For the cell shown, the measured cell potential, ?cell is −0.3723 V at 25 °C25 °C. Pt(s) |…

A: Half-cell reactions: H2(g) + 2e-  → 2H+(aq)    E0 = 0.00V Cd2+(aq) + 2e_  → Cd(s)  E0 = -0.403V…

Q: What mass of Cu(s) is electroplated by running 12.5 A of current through a Cu 2+ (aq) solution for…

A: We have to calculate the mass of Cu(s) is electroplated : First, we will write down all the given…

Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C.   Pt(s) |…

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Q: For the cell shown, the measured cell potential, ?cell, is −0.3723 V at 25 °C. Pt(s) | H2(g,0.773…

A: [ H+] = 0.091 M

Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current 6525 A flowing for a…

A: Given, Current = 6525 A or 6525 C/sTime = 50h = 50×3600 s = 180000seconds

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr, converting some of the H* to…

A: Given: Current (I) = 11.3 A     Volume of solution (L) = 1.25 L    Concentration of HBr = 0.552 M…

Q: Complete and balance the following redox reaction in basic solution O2(g) + Al(s) → H2O2(aq) + AIO2…

A: I hope we know the rules for balancing equation in basic medium. 1st all other elements except…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given: Concentration cell of hydrogen. Temperature = 298 K. Concentration of H+ in cathode = 1.00 M…

Q: How long will it take to plate out 0.270 g of iron metal from a solution containing Fe3+(aq) in an…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reaction…

Q: Which of the following reagents can oxidize H,0 to O2(g) under standard-state conditions? H*(aq), CI…

A: Given species: H2O and O2(g). Given oxidizing agents: H+(aq), Cl-(aq), Cu2+(aq), Pb2+(aq),…

Q: For each of the following reactions, complete and balance the equations taking place a. in acidic…

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Q: Assume molten ACI3 is electrolyzed with a current of 15.2 A. A3+ (aq) + 3 e¯ --> A (s) Eº = 1.04 V…

A: Faraday's law of electrolysis is given by Michael Faraday. Faraday's first law depicts that the…

Q: Complete and balance the following half-reaction in acidic solution As(s) → H:AsO. (aq) 1 2 3 4 5 6…

A: Note: Since we solve one question at a time, we’ll answer the first question as the exact one wasn’t…

Q: (a) A Cr* (aq) solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

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Q: Complete and balance the following redox reaction in basic solution.. 103 (aq) + S (aq) → 10 (aq) +…

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Q: Complete and balance the following redox reaction in basic solution Cr,0, (aq) + 1,(s) Cr* (aq) +…

A: Balance the half redox reaction using the steps At last add both and cancel out common term.  And…

Q: Balance the following redox reaction in acidic solution: MnO4 (aq) + Fe (s) Mn2* (aq) + Fe3+ --->…

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Q: Consider the following voltaic cell at 25°C: |3+ Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) |…

A: This problem is based on Nerst Equation For which, first we need to calculate the E°cell E°cell =…

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

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

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Q: Complete and balance the following redox reaction in acidic solution H2O2(aq) + Cr2O;² (aq) → O2(g)…

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Q: A galvanic cell is constructed in which the overall reac- tion is Cr,O} (aq) + 14 H¿O*(aq) + 6 I…

A: Reduction half reaction: Cr2O72- + 6e = Cr3+    [E0 (Cr2O72-/Cr3+) = 1.33 V] Oxidation half…

Q: How many hours does it take to form 15.0 L of O2 measured at 750 torr and 30°C from water by passing…

A: According to Faraday's first law ,when current is passed through an electrolytic solution, the…

Q: A current of 5.26 A is passed through a 2Sn(NO3)2 solution. How long, in hours, would this current…

A: In Sn(NO3)2 we have Sn in Sn2+ form  Hence to get tin that is Sn from Sn2+ the reaction will be Sn2+…

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.