Q: 2. Ate Shawol and Concertina performed electrolysis to determine the identity of an unknown metal X.…
A:
Q: 21.25 What is the difference between an active and an inactive electrode? Why are inactive…
A: Electrodes: In electrochemical cells, the electrodes are used as the conductors to supply the…
Q: 1. A constant direct current of 0.027 A flows through an silver coulometer for a period of 1 hour.…
A: The total charge, Qtotal, passed into the solution by the current is; QTotal=I×t=0.027 A×1 h×60 min1…
Q: .26 Which of the following metals can be used to cathodically protect iron? A. tin B. zinc C. nickel…
A: Solution [26.] : A process known as cathodic protection can be used to prevent rust formation,The…
Q: +. +. D(3147) Caught Dislocat 404-File or directory not f OWLV2 | Online teaching an…
A:
Q: Write the overall electrochemical reaction in the galvanic cell: Cu I Cu2+II Fe3+IFe2+ and…
A: Electrochemical Cell: The type of cell which converts chemical energy into electrical energy. In…
Q: A current of 0.941 amps is passed thru a soltion of Tl(III) until 0.319 g Tl metal is deposited.…
A:
Q: Calculate the mass of Cl₂ consumed if the battery delivers a constant current of 573 A for 60.0 min.…
A: All the above answer is correct so, solving only last part, the mass of Cl2
Q: A current of 3.22 A is passed through a Ni(NO,), solution. How long, in hours, would this current…
A: We have to calculate the time required.
Q: oblem Set #9 (Ch 19) rcise 19.42 – Enhanced – with Feedback 4 of 15 I Review I Constants I Periodic…
A: We have given that Ni(s) + 2H+(aq) -------> Ni2+(aq) + H2(g) the oxidation half reaction :…
Q: What is the potential generated by the battery. (Data: E ° of Pb (II) / Pb = -0.13V and Al (III) /…
A: To calculate the cell potential we have to use Nernst Equation Since we know that when the…
Q: 2. Why would a sacrificial anode made of lithium metal be a bad choice despite ts E•Li+/Li=-3.04 V,…
A: Sacrificial anode: Sacrificial Anodes are highly active metals that are used to prevent a less…
Q: 38. From the following data: Zn (aq/Zn(s) E° = -0.76V Fe" (aq)/ Fe" (aq) E = -0.77V It can be…
A: Reduction is defined as the gain of electrons whereas oxidation is defined as the loss of electrons.…
Q: 15. How many minutes would a current of 10.0 amps need to run through a solution containing Cut2 to…
A:
Q: What would the voltammogram for an irreversible reduction reaction look like?
A: In a cyclic voltammogram, the reversible reactions proceeds through electron transfer rate (at all…
Q: The F concentration of a solution was determined by measurements with a liquid-membrane electrode.…
A: Given, The initial potential is = 0.5021 volt Volume of sample is = 25 mL. Final potential is =…
Q: Part A- Construction of Voltaic Cells and Measurement of Cell Potentials Trial Trial 1 2 Zn/Pb Zn/Ni…
A: #Trial-2: Copper/Lead cell: Since Cu2+(aq) has higher reduction potential, it will undergo…
Q: 21. How many grams of Cu will be plated out by a current of 2.3 a applied for 25 minutes to a 0.50 M…
A: According to the Faraday's law of electrolysis The amount of an element deposited at an electrode is…
Q: Part A: Electrochemical Cell Mass Data for Electochemical Cell Copper Zinc Initial mass of strip…
A: a) Amount of Zn lost = 0.201 g Thus the theoretical amount of Cu gained must be = 0.201 g
Q: → Ni e → Fe 2 eH₂ + 2 OH™ e → Al e → Mg → Na Li roduced at the anode roduced at the cathode oduced…
A: In electrolysis, Cation moves toward cathode and reduced there . Anion moves toward anode and…
Q: 15. How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…
A:
Q: What current strength in ampere is required to deposit 500mg of Ni+2 from a Ni+2 playing cell of an…
A: Recall reaction for deposition of Ni from Ni+2 Ni+2+2e→Ni Recall Faraday's combined law…
Q: grams of Ag would be deposited by supplying an electric current of 0.50 A for 30 min
A:
Q: Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question. What is the…
A: The given cell is : Al(s)|Al3+||Cr3+|Cr(s) This cell is represented as : At the anode, oxidation…
Q: 17. What volume, in milliliters, of a 2.5% (m/v) KOH solution can be prepared by diluting 50 mL of a…
A:
Q: Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question. Which…
A: Since in the reaction, the Co2+ present in Co(NO3)2(aq) solution will convert to Co Hence Co2+ is…
Q: Using a current of 4.75 A, how many minutes does it take to plate onto a sculpture 1.50 grams of Cu…
A:
Q: General Chemistry 4th Edition McQuarrie • Rock Gallogly University Sci presented by M The voltage…
A: Lower the value of standard reduction potential, then the given electrode acts as anode and higher…
Q: Label the parts of the electrolytic cell for electrolysis of PbCl2 1: 2: 3: 4: 5: 6: 7: 8: Anode…
A: The addition of electrons or decreases in the oxidation state is known as a reduction reaction and…
Q: For an electrochemical cell to function you need both a path for electron flow and ion flow. In the…
A: An electrochemical cell is a device that converts chemical energy into electrical energy.
Q: b) What happens during electrolysis at anode and cathode electrode. Match up the boxes. 6 volt de…
A: Electrolysis is the process in which obtained purest form of metal from its ores. This process is…
Q: Record and calculate the missing data. Use the Level 0 and 1.0 M concentrations of the simulation.…
A: The chemical species having higher reduction potential undergoes reduction and acts as cathode The…
Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…
A:
Q: Talble li Voltai Calle Metale terted Metal at Metalat Eseli () Edel V) Anoho Cathode Cell 1.Zn°IZn…
A:
Q: d) The cell Mg(s) + Cd2(aq) Mg+ + Cd(s) has Ecell=+1.97 V. The magnesium electrode was dipped into a…
A: The given reaction is Mg(s) + Cd2+(aq) --------> Mg2+(aq) + Cd(s) E°cell = +1.97 V Ecell =…
Q: - Complete the table as follows: E Measured: Re-enter the values from Part A, Column 2 of the Report…
A: Cell potential of an electrochemical cell can be represented by following E cell = E cathode - E…
Q: A UPDATES AVAILABLE Do you want to install the updates now? Table 2 Half-Reaction Standard Reduction…
A:
Q: 1.b- A battery being charged at the finishing rate gives positive and negative electrode cadmium…
A: Cadmium reading taken on charge when the battery is at the end of charge can be vVery helpful in…
Q: Consider a ring which was electroplated with gold (Au, MM = 197 g/mol) using an Au(III) salt with a…
A: Given, A ring is electroplated with Au ( gold) using Au+3 salt with a 0.233 Ampere current for 7…
Q: Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard…
A:
Q: Part A If a voltaic cell is created betvween a Am?"/Am electrode and a Fe"/Fe electrode, what…
A: Voltaic cell is an eletrochemical cell that uses a chemical reaction which produce electrical…
Q: 2. Ate Shawol and Concertina performed electrolysis to determine the identity of an unknown metal X.…
A: we have to find the unknown metal X from the given values
Q: 670.24 sec
A: Given data are as follows: Weight of silver deposited = 1.5 g Current passed = 2A
Q: s: + electrons migrate e the Mn|Mn2+ electrode e the Pb ons migrate e the Pb|Pb²2+ compartment e the…
A: In electrochemical cell, Oxidation takes place at anode and reduction takes place at cathode. A)…
Q: Record the voltage for the Zn-Mg battery and compare this with the calculated voltage
A: Zn(s) + MgSO4(aq) no reaction The standard reduction electrode potential of Zn/Zn2+ is = -0.76 V…
Q: How long would it take to electroplate a flute with 28.3 g of silver (107.87 g/mol) at a constant…
A: Given-> Weight of Ag = 28.3 gm Atomic mass of Ag(MM) = 107.87 g/mole Current (i) = 2.0 ampere
Q: A baby'sspoon with an area of 6.25 cm2 is plated with silver from AgN03 using a current of 2.00 A…
A: (a),
Q: Rank the four metals (Cu, Zn, Pb, and Ag) in terms of ease of oxidation from easiest to hardest.
A:
Q: A mixture containing molten NiCl2 and SnBr2 undergoes electrolysis by passing a current between two…
A: A question based on electrolysis that is to be accomplished.
Step by step
Solved in 2 steps
- (c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?In the video "Sacrificial Anode Materials Demo", which among Zn, Al, Mg served as as i) sacrificial anodes? and ii) as noble coatings?Cathodic protection can be achieved by attaching a more (anodic / cathodic) material to the one to be protected.
- The E°cell = 0.135 V for the reaction3I2(s) + 5Cr2O72-(aq) + 34H+(aq) → 6IO3-(aq) + 10Cr3+(aq) + 17H2OWhat is Ecell if [Cr2O72-] = 0.014 M, [H+] = 0.21 M, [IO3-] = 0.00018 M, and [Cr3+] = 0.0039 M?Ecell =For the reaction, 2CuI(s) + Cd(s)--->Cd2+ + 2I-(aq) + 2Cu(s), E0=0.23V. Given that E0Cd2+/Cd=-0.403V, determine E0 for the half reaction.At 25 ∘C,25 ∘C, a titration of 15.00 mL of a 0.0320 M AgNO3 solution with a 0.0160 M NaI solution is conducted within the cell SCE || titration solution | Ag(s)SCE || titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of NaINaI solution? The reduction potential for the saturated calomel electrode is ?=0.241 V. The standard reduction potential for the reaction Ag++e−⟶Ag(s) is ?∘=0.79993 V The solubility constant of AgI is ?sp=8.3×10^−17. 0.200 mL?= 19.00 mL?= 30.00 mL?= 43.20 mL?= please solve
- the fpllowing cell was used fordetermination of pCrO4: SCE||CrO4^2-(xM),Ag2CrO4(sat'd)|Hg calculate the pCrO4 IF THE POTENTIAL is -0.313V.The _____ in a _____ voltammogram is related to the ____ a. limiting current, cyclic, concentration of the analyte of interest b. limiting current , linear sweep, concentration of the analyte of interest c. peak current cyclic, standard reduction potential of the analyte of interest d. peak current , linear sweep, standard reduction potential of the analyte of interest e. none of theseFor Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 4. Why is it necessary to carry out the reduction of iron and then the titration, before going on to the next sample 5. If you look carefully, there are pieces of tin metal on the bottom of the SnCl2 reagent solution. Why is it there?
- For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 1. What is the purpose of the phosphoric acid in this experiment? Please be specific. 2. How does the Diphenylamine sulfonate indicator work? What chemical reaction causes the color change? How is an indicator chosen in a redox reaction?For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 3. How would you prepare a complete anlaysis procedure using KMnO4 as the oxidant instead of K2CrO7? Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular what is the purpose of the Zimmerman Reinhardt Reagent?Calculate the pH of a 0.01M HNO3 solution taking into account activity.