A galvanic cell is constructed that has a zinc anode immersed in a Zn(NO3)2 solution and a platinum cathode immersed in an NaCl solution equilibrated with Cl2(g) at 1 atm and 25°C. A salt bridge connects the twohalf-cells.(a) Write a balanced equation for the cell reaction.(b) A steady current of 0.800 A is observed to flow for a period of 25.0 minutes. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to?(c) Calculate the change in mass of the zinc electrode.(d) Calculate the volume of gaseous chlorine generated or consumed as a result of the reaction.

Q: The electrolysis cell shown here was run at a constant current of 0.021 96 A. On one side, 49.22 mL…

A: (a) The volume of H2 gas produced at STP is calculated using the combined gas law as shown below,…

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: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo; (aq)…

A:

Q: a) Balance the following reactions.  b) Calculate the cell potential and the Gibbs free energy of…

A: For each reaction cell potential, gibbs free energy, redox reactions and line representation of…

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

A:

Q: A current of 4.21 A is passed through a N i ( N O 3 ) 2 solution. How long, in hours, would this…

A: Current (I) = 4.21 A  Mass of nickel deposited (m) = 4.50 g

Q: one process used for electroplating silver, a current of 10.23 A was passed through an electrolytic…

A: Electroplating is a process in which a thin layer of one metal is deposited on another metal surface…

Q: 3. (a) Liquid NH3 is subjected to electrolysis. One of the half-reactions is 2 N3 N₂+6 e How many…

A: Given data:The given reaction is :a) How many faradays of electricity are required to produce 4.12 L…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

A:

Q: Answer the following questions by selecting the appropriate half-reaction. Assume that in each case…

A: NOTE : Since you've posted a question with multiple sub-parts,we'll solve first three sub-parts for…

Q: A galvanic cell consists of a cathode with a nickel electrode in a 0.186 M solution of Ni(NO3)2 and…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

A:

Q: How many minutes will it take to electroplate 32.1 gg of gold by running 5.00 AA of current through…

A: Au+   +   e-    ------> Au   1 mol of Au requires 1 mol of electron 1 mol of electron = 96485 C…

Q: In a galvanic cell, one half-cell consists of a tin strip dipped into a 1.00 M solution of Sn(NO3)2.…

A: Given , Cell voltage = 0.595 V

Q: Manganese metal can be produced industrially by electrolysis of MnO2. How many hours would it take…

A: The compound of manganese electrolysed is MnO2 having Mn4+ ion. Hence the electrolysis reaction to…

Q: Calculate the mass of cobalt plated onto the cathode of an electrolytic cell by a current of 15.0 A…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction   Ti(s)+Co2+(aq)↽−−⇀…

A:

Q: A concentration cell is set up by connecting a half-cell containing a lead electrode in 0.10 M…

A:

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: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) Ti² (aq) +…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+…

A: In an electrochemical cell, the chemical energy due to the chemical reactions is converted into…

Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq) using a…

A:

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: given data are-  Fe(s) ⟶ Fe2+(aq) + 2e-Eo = -0.44 V  O2(g) + 4H+(aq) + 4e- ⟶  2H2O(l)  Eo = 1.23 V…

Q: The following galvanic cell has 8° = +1.887 V at 25°C: Co(s) | Co2+ (aq) || Ce4+ (aq), Ce3+ (aq) |…

A: The solution is as follows:

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: galvanic cell is constructed in which a Pt | Fe2+ Fe3+ half-cell is connected to a Cd2+ | Cd…

A:

Q: (a) How long (in hours) does it take to produce 454 g of copper from a solution containing Cu²*…

A: Given: The mass of copper to be produced from Cu2+ = 454 g We have to find the amount of energy (in…

Q: Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature and…

A: Given information: Current = 12.4 A Time = 1.0 h Charge flown:  Q = It= 12.4×60×60= 44640 C For the…

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…

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.