A voltaic cell consists of a strip of cadmium metal in a solution of Cd(NO3)2 in one beaker, and in the other beaker a platinum electrode is immersed in a NaCl solution, with Cl2 gas bubbled around the electrode. A salt bridge connects the two beakers. Which electrode serves as the anode, and which as the cathode? I thought it was the Cd acting as cathode and Pt as anode, but I am having a hard time with this problem conceptually.

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Fe(s)+ PdCl2(aq)→…

A: Suppose the galvanic cell sketched below is powered by the following reaction:   Fe(s)+ PdCl2(aq)→…

Q: In the electrolysis of a solution containing Ni2 + (aq), metallic deposits Ni(s) on the cathode.…

A: The problem is asking us to calculate the mass of nickel that will form on the cathode during…

Q: Use the standard reduction potentials shown here to answer the questions. A copper, Cu(s), electrode…

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Q: Answer the following questions about this cell. If you need any electrochemical data, be sure you…

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Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: For cell Ni|Ni2+||Ag+|Ag At anode- Ni(s) -----> Ni2+(aq) + 2e-       ∆E° = 0.23 V At cathode-…

Q: A voltaic cell is set up with copper and hydrogen half-cells. Standard conditions are employed in…

A: Given :  Ecell = 0.49 V  PH2 = 1 atm  [Cu+2] = 1 M

Q: A certain metal M forms a soluble nitrate salt MNO 3. Suppose the left half cell of a galvanic cell…

A: Let's carefully re-examine the calculations to ensure the answers are accurate. Step 1: Identifying…

Q: student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

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

Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

A: Given,  Concentration of MNO3 in left half = 22.5 mM  Concentration of MNO3 in right half = 4.50 M…

Q: a current of 5.79 A is passed over 500 seconds in 300 ml of aqueous solution of copper sulphate…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction:…

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Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Faraday's law states that the amount of chemical change that is produced by passing a current to an…

Q: A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: The Faraday’s first law of electrolysis state that the mass of the substance  deposited at any…

Q: A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a…

A: A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a…

Q: When we have an inactive electrode like Pt(s) in a galvanic cell as the cathode, what does it…

A: To explain: The role of platinum as an electrode.

Q: what mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

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Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A: For a cell   Cell potential = E°Reduction half  - E°Oxidation half Species whose reduction potential…

Q: 14.106 A voltaic cell is constructed in which the following reaction takes place: Cu (s) + 2Ag+ (aq)…

A: Number of moles of a substance is defined as ratio of mass in gram of substance to the molar mass of…

Q: 5. Consider the following galvanic cell at 298 K. B(s) | B*(0.0050 M) || A²*(0.0100 M)| (s) A2+(aq)…

A: We have given  Consider the following galvanic cell at 298 K. B(s) | B+ (0.0050 M) || A2+ (0.0100 M)…

Q: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

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Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…

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Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

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Q: Like any piece of apparatus, an electrolytic cell operates at less than 100% efficiency. A cell…

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Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Given that : A student constructs an electrochemical cell with a half-cell composed of a nickel…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Cl₂(g)+2e 2 CI…

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Q: A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a…

A: Electrochemical cell is a cell in which chemical energy is converted to electrical energy. It is…

Q: A concentration cell containing aqueous solutions of Cu(NO3)2 and solid copper metal is constructed…

A: The cell reaction for the concentration cell is Cu2+(aq) (higher concentration)→Cu2+(lower…

Q: Consider the following electrochemical cell reaction:   Pb2+(aq)  +  2 Cr2+(aq)  →  Pb(s)  +  2…

A: We will calculate cell potential using nernst equation.

Q: A galvanic cell is powered by the following redox reaction: Cl,(g) + H,(g) + 2 OH (aq) → 2 Cl (aq) +…

A: Given : We have to write half reaction taking place at anode and cathode.

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is…

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Q: A voltaic cell utilizes the following redox reaction and operates at 298 K: 3 Ce¹+ (aq) + Cr (s) → 3…

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Q: Sketch the galvanic cell based on the following overall reactions. Calculate e°; show the direction…

A: The standard reduction potentials of the two half-cells are: Cl2/2Cl-: 1.36 VCr2O72-/Cr3+:1.33 V

Q: A cell is set up with copper and lead electrodes in contact with CuSO4(aq), and Pb(NO3)2(aq). If…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Se have to find out the total no. of transferring electron

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

A:

Q: A galvanic cell is powered by the following redox reaction: 3 Cl,(9) + 2 Cr(OH),(s) + 10 OH (aq) 6…

A: The overall reaction taking place is given as,

Q: MnO 4(aq)+8H (aq) +5e 3+ 2+ Fe³+ (aq) + e → Fe (aq) Answer the following questions about this cell.…

A: From the given data, we need to identify the reaction at cathode, anode.

Q: A galvanic cell is powered by the following redox reaction: Br, (1) + H,(g) + 2 OH (aq) - 2 Br (aq)…

A: We have to write half-cell reaction on both anode and cathode electrodes and find the standard cell…

Q: We construct a cell in which identical copper electrodes are placed in two solutions Solution A…

A: The electrode at which the concentration of Cu2+ is 0.75 M acts as a cathode and another electrode…

Q: Suppose a powerful battery is connected between a pair of inert graphite electrodes dipped into a…

A: An electrode is an electrical conductor used to make contact with a nonmetallic part of a circuit.…

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

A: Given: Mass of god produced = 0.34 g. Current passed = 0.10 A

Q: A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a…

A: The electrochemical cell that utilized energy released from spontaneous chemical reaction to produce…

Q: A certain electrolytic cell produced 39.0 g Cl, from molten NaCl. The time it took for this process…

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Q: the metal in the electrolysis solution

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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.