8. Which of the following reactions is a redox reaction? A) 2HCl + Ca(OH)2 → CaCl2 + 2H₂O B)CaCO3 → CaO + CO2 C) HCl + AgNO3 → AgCl + HNO3 D) 2PbO2 → 2PbO + 0₂ E) NaHCO3 + H₂SO4 → Na2SO4 + CO₂ + H₂O
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- A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.76 V, and Δ?∘???ΔGrxn∘ = −134 kJ/mol. If the concentration of Zn2+ is increased to 2.0 M, then ?????Ecell will ______ and Δ????ΔGrxn will be _________ than Δ?∘???ΔGrxn∘. Zn(s) + 2H+(aq) ⟶⟶ Zn2+ + H2(g) Group of answer choices decrease, less negative increase, more negative increase, less negative decrease, more negativeZinc plating (galvanizing) is an important means of corro-sion protection. Although the process is done customarily bydipping the object into molten zinc, the metal can also be elec-troplated from aqueous solutions. How many grams of zinc canbe deposited on a steel tank from a ZnSO4 solution when a 0.855-A current flows for 2.50 days?When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate PbSO4 is reduced to lead at the cathode and oxidized to solid lead(II) oxide PbO at the anode. Suppose a current of 59.0A is fed into a car battery for 66.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol
- A certain metal M forms a soluble sulfate salt MSO4 . Suppose the left half cell of a galvanic cell apparatus is filled with a 20.0mM solution of MSO4 and the right half cell with a 4.00M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0°C. Which electrode will be positive? left or right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.A certain metal M forms a soluble sulfate salt M2SO4 . Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of M2SO4 and the right half cell with a 2.50mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0C.Fill in the following brackets: Redox reactions can also lead to greenhouse gas emissions from soils. Under very strongly reducing conditions (Eh < -0.1) the dominant GHG released from soils is likely ["carbon dioxide", or "methane", or "nitrous oxide", or "nitrous oxide and carbon dioxide"], whereas, at oxidizing conditions (Eh > +0.2) release of ["carbon dioxide", or "methane", or "nitrous oxide", or "nitrous oxide and carbon dioxide"] is more favorable.
- An aqueous solution of an unknown salt of ruthenium Is electrolyzed by a current of 2.70A passion for 20.0min. If 1.132g of Ru is produced at the cathode, what js the charge on the ruthenium ions in solution?The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell. Result: a) Eºcell >0 d) 0.7108 V, 0.7482 VCopperplating is a technique in which copper metal is deposited electrolytically on a surface to enhance conductivity and reduce Using a current of 4.75 A, how many minutes does it take to plate 1.50 g of copper metal onto a metal piece from a CuSO4 solution?
- When an aqueous solution of CuSO, is electrolyzed copper metal is deposited. If a constant current was passed for 5.00 h and 404 mg of Cu (63.546) metal was deposited, what was the current?a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of current pass through an electrolytic cell with an NiNO3 electrode solution for 5.00 hours? Faraday’s Constant = 96,500 Coul/mol e-Ni+(aq) + e- ---->Ni (s) b) To plate a dental explorer with 10.00 g of Nickel (58.6934 g/mol) from a NiNO3 aqueous solution, a metallurgist utilized a 5.00 amp current. How long will it take in minutes, to plate out 10.00 g of zinc? Ni+(aq) + e---->Ni (s)A student was asked to set-up a galvanic cell in the laboratory. He used two copper electrodes, one with an electrolyte solution of lower concentration. He then connected the two electrodes by a conductive wire with a voltmeter. However, he noticed that the reaction eventually stopped as there was no longer a voltage reading. What caused the halting of the reaction? a. The use of identical electrodes for the anode and cathode. b. The build-up of charge due to absence of salt bridge. c. The presence of the voltmeter in the circuit. d. None of the above.