O Fe(ag) The balanced half-reaction occuring at the cathode in the redox reaction shown below is 3Mnoalag) +24H) + 5Fe(s) → 3Mn? +5Fe + 12H2O) eTag) + 12H2Ou O Fe +3e → Fe(s) O Fels + Fe + 3e → Fet +3e F(aq) O Mnoalao) + 8H) + 5e-+ Mn + 4H200 '(aq) '(aq) O Mn + 4H2Oo→ MnOalaq) + 8Hag) + 5e¯ + 8H+ 5e- '(aq)

Q: According to the cell notation below, a galvanic cell is made up of a magnesium electrode and a…

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Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: How much  Na(s)Na(s) and Cl2Cl2 can be produced

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Q: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

Q: In an experiment of a redox reaction, an electrochemical cell has been set up by connecting a vessel…

A: Hello. Since the question contains multiple subparts, the first three subparts are solved. In case…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Hg metal…

A: Redox reaction - it is also known as  oxidation- reduction reaction.  It is a type of chemical…

Q: All WOTK men A solution of NaCl (aq) is electrolyzed for 15.5 min using a current of 3.45 A. Write…

A: Given that, a solution of NaCl (aq) is electrolyzed. The time is t = 15.5 min = (15.5×60) sec = 930…

Q: Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq)

A: The answer to the given question is as follows.... First we equate the number of respective atoms on…

Q: During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.…

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Q: How many seconds are required to produce 8.00g of aluminum metal from the electrolysis of molten…

A: Assume that the required seconds as x. 1 A = 1 C/s. Coulombs generated by 12.0 A in x seconds is 12…

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

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Q: For the following balanced redox reaction under basic conditions: 3 Zn(OH)2 (s) + 2 Cr(OH)3 (s) + 4…

A: We will first calculate E° cell , then using it we will predict the correct statements

Q: )Calculate the equilibrium constant for the following balanced redox reaction at 298 K: O2(g) +…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: In an experiment of a redox reaction, an electrochemical cell has been set up by connecting a vessel…

A: Given, Eo (Sn2+/Sn) = -0.14 V Eo (Ag+/Ag) = +0.80 V Concentration of Sn2+= 0.50 M Concentration of…

Q: The cathode is the electrode at which oxidation occurs. O True O False

A: We are authorised to call for the one question at a time. Please post the other question separately.

Q: current

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Q: Hydrazıne, N2H4, has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing…

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Q: What amount of Cu (in grams) is deposited at the cathode when a current intained for 15 minutes in a…

A: Faraday's second law of electrolysis explains that when a certain amount of charge is passed, the…

Q: Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the…

A: Ecell can be calculated using nernest equation.  For this first we write reduction and oxidation…

Q: Gold can be plated out of a solution containing Au3+ according to the half-reaction:Au3+(aq) + 3…

A: It is given that gold is plated for 25 minutes and the current is of 5.5 A and the half-reaction is…

Q: 2. (m) A galvanic cell is assembled using the AgIAg' and Al|AP" electrodes. Identify the cathode and…

A: The cell potential of an electrochemical cell is the potential difference occurring between the two…

Q: In the commercial preparation of aluminum, aluminum oxide, Al2O3, is electrolyzed at 1000°C. (The…

A: Given- mass of aluminum = 3.09 kg Reaction Al3+ + 3e- ----> Al To find- coulombs of electricity…

Q: An electrochemical cell is constructed according to the line notationPt | Sn2+ (1.00 M), Sn4+ (1.00…

A: Electrochemistry is the branch of chemistry that studies the change of chemical energy into…

Q: The electrolysis of molten AIClz for 4.25 hr with an electrical current of 25.0 A produces g of…

A: The amount of Aluminum produced can be calculated as follows

Q: 1. The following redox reaction was constructed at 25.0°C. Pb²+ (aq) + Mg(s) → Pb(s) + Mg² (aq) a.…

A: The given reaction is :  Pb2+ (aq) + Mg (s) ----------> Pb (s) + Mg2+ (aq)  d. As the reaction…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Co metal…

A: Interpretation: We have to write the reaction between Co metal and F2(g)

Q: How much time in minutes would it take to deposit 1.65 grams of X (MW = 68.43 g/mol) on a cathode in…

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Q: A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at…

A: Given: Time passed = 31.5 hr = 31.5 × 3600 = 113400 s                             (Since 1 hr = 3600…

Q: A solution of a metal ion Mag is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g of…

A: a.

Q: A certain half-reaction has a standard reduction potential E=+0.51 V. An engineer proposes using…

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Q: A current of 0.4 Amps flows for 2 hours through an electrolytic cell containing copper sulphate…

A: This problem can be solved by using Faraday's first law of electrolysis accordingto which weight of…

Q: Electrolytic process of determining molar mass.  An electrolysis cell contains X3+ ions. When a 5.45…

A: In a electrolytic process, cations go to the anode and anions go to the cathode.

Q: A galvanic cell is powered by the following redox reaction: 2 Cu*(aq) + H,(9) + 2OH (aq) - 2 Cu*…

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Q: . Electrodepositing all the Cu and Cd from a solution of CuSo, and Cdso, required 1.20 F of…

A: The two half-reactions are as follows:  Cu2+ + 2e- → Cu Cd2+ + 2e- → Cd Let us assume that x is mol…

Q: In an  electrolysis experiment a student passes the same quantity of electricity through two…

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Q: How much current should pass through

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Q: 1. A solution of a metal ion Mi) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g…

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Q: Electrolysis of molten  NaClNaCl is done in a Downs cell operating at 7.0 volts (V) and 5.0×104 AA .…

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Q: equilibrium constant

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Q: Electrolysis of molten CaCl2 is carried out in an electrolysis cell. If 0.904 ampere current is…

A: Molten CaCl2 is electrolysed by 0.904 ampere current during 3 hours. During electrolysis of molten…

Q: How long will it take in hours to create 1.026 grams of Cr at the cathode of an electrolytic cell if…

A:

Q: The electrolysis of CUCI(ag) produces Cu(s) and Cl2(g). What is the minimum external emf needed to…

A: Standard reduction potential of Cu+/Cu = 0.52 V Standard reduction potential of Cl2/Cl- = 1.36 V

Q: A galvanic cell is powered by the following redox reaction: 3+ NO3(aq) + 4H* (aq) + 3 Fe²+ (aq)…

A: Known: EFe3+|Fe2+o=0.771 VENO3-|NOo=0.957 V

Q: In the electrolysis of a solution containing Ag* (aq), metallic Ag(s) deposits on the cathode. Using…

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Q: Calculate the time to deposit 1.27 g of copper at cathode when a current of 2 A was passed through…

A: According to Faraday's first law W = z.i.t                                        .....(1) W is the…

Q: Consider the unbalanced redox reaction: Cr,0;,"(aq) + Cu(s) – c²*(aq) + Cư**(aq) Balance the…

A: The given reaction is balanced as follows - Cr2072- (aq) + Cu (s) → Cr+3 (aq) + Cu+2 (aq) Step: 1…

Q: Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the…

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Q: Electrolysis of molten  NaCl is done in a Downs cell operating at 7.0 volts (V) and 4.0×104 A . How…

A:

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.