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- What is the equilibrium constant (K) at 25°C for the following cell reaction? Co(s) +Ni2+→Ni(s)+ Co2+ Group of answer choices 1.39x1018 5.7x106 9.7 2.7 6.5 Open link to see table https://openstax.org/books/chemistry-atoms-first-2e/pages/16-3-electrode-and-cell-potentials#fs-idm42585168Give only typing answer with explanation and conclusion The following reaction takes place in the lead-acid battery ("car battery"): PbO2 + Pb + 2HSO4 2PbSO4 + 2H2O Calculate how many kg of Pb are converted to PbSO4 when a 55 Ah battery is completely discharged PbSO4 (M_Pb = 207 g mol-1).A 1 M solution of Cu1NO322 is placed in a beaker with astrip of Cu metal. A 1 M solution of SnSO4 is placed in asecond beaker with a strip of Sn metal. A salt bridge connects the two beakers, and wires to a voltmeter link the twometal electrodes. (a) Which electrode serves as the anode,and which as the cathode? (b) Which electrode gainsmass, and which loses mass as the cell reaction proceeds?(c) Write the equation for the overall cell reaction. (d) Whatis the emf generated by the cell under standard conditions?
- 1. Consider a cell buffered at pH 2.00 and consists of Fe2+(aq) (0.004 M), Fe3(aq) (0.070 M) and MnO4-(aq) (0.024 M), Mn2+(aq) (0.050 M), in which Fe2+ reduces MnO4- to Mn2+. a. Write the balanced reactionb. What is the standard cell potential? Is the cell galvanic or electrolytic?c. What is the actual cell potential at 35.0oC?A Cu electrode is immersed in a solution that is 1.00 Min [Cu(NH3)4]2+ and 1.00 M in NH3. When the cathodeis a standard hydrogen electrode, the emf of the cell isfound to be +0.08 V. What is the formation constant for[Cu(NH3)4]2+?A solution is 10^-3 M in Cr2O72- and 10^-2 M in Cr3+ . If the pH is 2.0, what is the potential of the half reaction at 298K? Cr2O72- + 14H+ + 6e- ↔ 2Cr3+ + 7H2O
- 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. From the reaction as shown below, calculate the Standard Cell Potential of a Galvanic Cell that uses the half-reactions shown below. Cr3+ + 3e- -------> Cr Eo = -0.73 V Al3+ + 3e- -------> Al Eo = -1.66 V B. A galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V at 50oC. What is the concentration of CuSO4 in the cathode compartment? Zn(s) + Cu(aq)2+ -------> Zn(aq)2+ + Cu(s) Eo = 1.10 V Use:E = Eo - (RT/nF) + lnQA galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.25 V, and ΔGrxn∘ = −44 kJ/mol. If the concentration of Ni2+ is increased to 2.0 M, then Ecell will ______ and Δ????ΔGrxn will be _________ than ΔGrxn∘. Ni(s) + 2H+(aq) ⟶⟶ Ni2+ + H2(g) A) decrease, less negative B) decrease, more negative C) increase, less negative D) increase, more negative
- 4 If the glass and reference electrode are immersed in a buffer solution pH = 3.56 ,the electrode voltage was = -0.111V. when the two electrodes immersed in unknown solution , it was found that the voltage of the glass electrode = -0.041V. Calculate the pH of the unknown solutionUnknownOchem help with prelab The experiment is attached and involves the reduction of a nitro group to an amine The Chemicals are: 200 mg of m-nitroacetophenone 400 mg of granular tin 4 mL of 6M hydrochloric acid 30% sodium hydroxide Need help with the prelab which requires... A. Write the balanced equations for both half-reactions of the redox and then the overall balanced redox equation B. Determine the limiting reagent and the theoretical yield of amine1. How many gram of rach metal will be deposited assuming only cathodic reactionin each cell? Exactly 0.6 faraday electric charge is passed through threeelectrolytic cells in series, first containing AgNO3, second CuSO4 and third FeCl3solution. 2. Calculate the volume of chlorine gas liberated at the electrode at NTP if theelectric current of 110 ampere is passed through a molten liquid ofsodium chloride for 5 hours and 30 mins. 3. Density of silver is 10.5 g/cm 3 .How long has a current of 4 amperes to be appliedthrough a solution of silver nitrate to coat a metal surface of 80 cm 2 with 0.005 cmthick layer? 4. What current strength in ampere will be required to liberate 15 g of chlorine fromsodium chloride solution in one hour and a half? 5. What will be the molarity of the solution at the end of electrolysis and what will bethe molarity of solution if nickel electrodes are used if a current of 3.7 ampere ispassed for 6.5 hours between platinum electrodes in 0.56 litre of a 2 M…