Choose the species that is/are stable in a reducing environment at pH=10.

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀…

A: Given: The concentration of Ti2+ is 0.00180 M.The concentration of Co2+ is 0.813 M.The half-cell…

Q: The following standard reduction potentials have been determined for the aqueous chemistry of…

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Q: Balance the following reaction under acidic conditions and calculate cell potential at 298K Cr2O72-…

A: Calculate  cell potential Using  Nerenst  equation

Q: 7. Determine the cell potential (in V to two decimal places) for the following electrochemica cell:…

A: Given that an electrochemical cell is Cu(s)|Cu2+(aq, 0.02 M)||Cu2+(aq, 0.50 M)|Cu(s). We have to…

Q: The Faraday constant is 96500 Coulombs/mole e-.. Find the electronic charge; use the relation: 1 mol…

A: Faraday is a measure of electric charge. It is defined as the charge carry by  one mole of…

Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

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Q: Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

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Q: Molten RbCI can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

A: Given data: Weight of Rb = 23.4 g Current (A) = 1.25 A Equivalent weight of Rb = 85.461=85.46 Time…

Q: The standard reduction potentials of the Sn2"/Sn and Ag*/Ag couples are -0.14V and +0.80 V,…

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Q: Calculate the electromotive force for the galvanic element composed of electrodes: Pt, H2 (1 atm) |…

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Q: 15. Calculate AG° for the following galvanic cell: Mn(s) I Mn²*(aq) || Fe2+(aq) IFe(s), given these…

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Q: at a temperature of 25 ° C the galvanic element Pt | ClO3- 0,001M, Cl- 0,01M pH = 3 || Mn2 + 0.0001M…

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Q: As the concentration of an acid solution decreases, the cell potential (in V) also decreases. Why?…

A: The Nernst equation is used to calculate the potential of a half-cell in an electrochemical cell at…

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: The voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Q: The major products A, B, and C of the following scheme are: if R Me R PHCH₂OH (1 equiv) cat. H',…

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Q: Consider the following half reaction NO3(aq) + 10 H+ (aq) + 8e -> NH4+ (aq) + 3H₂O(1) If the ratio…

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Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: he voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

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: Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A…

A: Given: Current = 4.5 A The atomic weight of Cu =63.55 gThe atomic weight of Br2=159.8 gCharge of 1…

Q: Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an…

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Q: a) Nickel is immersed in 0.1M NaCl at pH = 1 and H2 pressure of 1 atm.  Calculate the potential of…

A: To solve the questions regarding the electrochemical potentials involving nickel, we'll examine both…

Q: A certain half-reaction has a standard reduction potential Ered=-1.18 V. An engineer proposes using…

A: The standard reduction potential at the cathode  = -1.18 V       The standard cell potential must be…

Q: The potential (EMF) of a corrosion cell consisting of zinc (Zn) and hydrogen (H2) electrodes…

A: The concept of given question is based on the Nernst equation.The Nernst equation can be used to…

Q: Molten RbCI can be electrolyzed to form metallic Rb. For what duration should an electrolysis be…

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Q: [References] Using values from the table of standard reduction potentials, calculate the standard…

A: We can solve this problem by using following equation ∆G° = -n×F×E° n = change no of electrons F =…

Q: Consider Zn+2 (0.056 M) | Zn || TI*3 (9.86 x 102M) I TI* (0.048 M) Pt E° (Zn*2/ Zn) = -0.763 V E°…

A: On the left half of the cell representation there is anode and on the right it is the cathode. Ecell…

Q: Nickel is immersed in 0.1M NaCl at pH = 1 and H2 pressure of 1 atm.  Calculate the potential of the…

A: To calculate the potential of the cathodic half-reaction when nickel is immersed in a 0.1 M NaCl…

Q: Calculate the concentration of the zinc sulfate solution using the Nernst equation. The Nernst…

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Q: For the reaction 2Co (aq) +201 (aq)-2Co²+ (aq) + Cl (s). E-0.483 V what is the cell potential at 25…

A: Answer: Cell potential will be calculated using Nernst equation which is shown below:…

Q: [References] Using values from the table of standard reduction potentials, calculate the cell…

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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: Calculate the time required to precipitate 200 milligrams of copper by electrolysis of an acidic…

A: By 1F of charge 1 equivalent of metal can be deposited .

Q: The voltaic cell Ca(o)Ca²+ (aq) || Ni?+(1.0 M)|Ni(s) has a cell potential of 0.300 V at 25°C. What…

A: Given : Ecell = 0.300 V Temperature = 25 oC Concentration of Ni2+, [Ni2+ ] = 1.0 M And Eocell =…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + With(so much) =…

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Q: How many liters of O2 at 298 K and 1.00 bar are produced in 2.75 hr in an electrolytic cell…

A: given: Pressure (P) = 1.00 bar temperature (T) = 298 K Time (t) = 2.75 hour x 3600 = 9900 sec…

Q: Predict the products of the electrolysis of an aqueous solution of sodium chloride in cell using…

A: Electrolysis is a spontaneous redox process Here we are required to find the product when aqueous…

Q: (a) Following reactions occur at cathode during the electrolysis of aqueous copper (II) chloride…

A: In the reduction, the oxidation state of an element is decreased to its lower value. In the…

Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…

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Q: The redox potentials for the Zn2+/Zn and Cl2/Cl– couples are -0.764 V and 1.395 V, respectively.…

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Q: E° and the Equilibrium Constant 2.) Example: Calculate the equilibrium constant (K) for the…

A: The oxidation and reduction half cells with standard electrode potential will be

Q: Determine the cell potential for a galvanic cell composed of copper and zinc at standard condition.

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Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: The voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Q: (a) Predict the products of electrolysis in each of the following:(i) An aqueous solution of AgNO3…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: The voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Q: Given the hypothetical metal samples a, B, and y were placed in an electrochemical cell as…

A: Answer: Standard cell potential can always be calculated using standard half cell reduction…