It took 2.13 min with a current of 2.18 A to plate out all the silver from 0.250 L of a solution containing Ag+. What was the original concentration of Ag+ in the solution?

Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

A: Given reaction is  Au3+ (aq) +   3e-    →  Au (s) According to Faraday's law, equivalent weight of a…

Q: Ag | AgCl (sat’d) |NaCl (0.1 M) || KI (x M) | 12(s) | Pt

A:

Q: What is the standard cell potential for a galvanic cell that uses the Zn/Zn" and the Ag/Ag" couples…

A: The term standard reduction potential for a given galavanic cell can be termed as the tendency of…

Q: (b) A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: 7. For each of the following reactions Write the oxidation and reduction half reactions Determine…

A: Oxidation involves loss of electrons whereas reduction involves gain of electrons.

Q: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

A:

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.05 minutes for a current of 1.91 A to plate…

A:

Q: It took 2.46 min with a current of 2.03 A to plate out all the silver from 0.250 L of a solution…

A: Applying formula w=Zit

Q: A constant current of 9.25 amperes is passed through a cell containing iridium (III) nitrate,…

A: We have current as 9.250 A , time as 7.57 hrs, deposit of Ir is taking place, we have to calculate…

Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

A:

Q: A current of 0.452 A is passed through an electrolytic cell containing molten CaCl2 for 1.50 hours.…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

A:

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the cathode…

A: Salt bridge is a laboratory device used to connect the two half cells by which we can connect the…

Q: If a salt bridge contains KNO3 as its electrolyte, which ions diffuse into solution in the anode…

A: A galvanic cell is an electrochemical cell that is used to supply electric current through the redox…

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A:

Q: Using a constant current of 7.8 A, a metal object is to be gold-plated by an electrolytic procedure…

A:

Q: A current of 4.15 A is passed through a Pb(NO3)2 solution for 1.50 h. How much lead is plated out of…

A: Given that:  Current(I) = 4.15A = 4.15C/s  Time(t) = 1.50h = 1.50h×3600s/h = 5400s Reaction:  Pb2+ +…

Q: A constant current of 3.20 A is used to deposit zinc on a cathode. How much zinc can be deposited in…

A:

Q: Determine the molar mass (AMU) of Metal (M) if it took 2.56 minutes for a current of 1.11 A to plate…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: A galvanic cell is constructed using two half-cells in standard state: Al|Al3* and Ni|Ni 2 Al (aq) +…

A:

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: How many seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

A:

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A: Mass can be calculated as:-

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

A:

Q: 7. For each of the following reactions Write the oxidation and reduction half reactions Determine…

A:

Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The metal deposited or liberated is given by the Faraday's first law of electrochemistry which is…

Q: Fe | Fe²+ (0.100M) || Cd²+(0.001) | Cd I. Write the half-reactions and cell reaction 2. Calculate…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current of 1 A to plate…

A: From combination of first and second law of Faraday, we have :  M = n*F*m/(I*t) ....(1) Here, n =…

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: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A:

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

Q: Pd2* + 2e → Pd(s) E° = 0.915 V Cu* + 1e 4 Cu(s) E° = 0.518 V а. Write the overall spontaneous…

A: Use relation of equilibrium constant and standard electrode potential.

Q: What is the Eθ cell value for a galvanic cell constructed using aluminium and nickel electrodes.

A: Foe finding Standard EMF of cell, we must know about the standard reduction potential values for the…

Q: 3.2 calculate the standard cell potential of the following cell at 250 Sn(s)|Sn*(aq)||Cu*(aq)|Cu(s)…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell…

A: Given : Current passed = 0.20 A And time = 1 min

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) +2Ag*(0.100 M)…

A:

Q: 12 The standard cell potential for the following galvanic cell is 0.71 V.…

A: Given- Standard cell potential of galvanic cell =0.71V Mg(s)|Mg2+(aq)||Al3+(aq)|Al  Equilibrium…

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given data:  Current = 4.57 A  Cr deposited = 14.5 g  Molar mass of Cr = 52 g.mol-  CrCl3  ==>…

Q: How many grams of  zinc metal will be deposited from a solution that contains  Zn^2+ ions if a…

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: How many minutes would a current of 20.0 amps need to run through a solution containing Au*3 to…

A: Amount of the current flow = 20A Mass of liberated substance = 10g Electron transfer per ion = 3

Q: How many minutes would it take to deposit all the  Al from 225 ml of 0.10 M   aluminum nitrate  with…

A: The given data contains, Molarity = 0.10 M. Volume = 225 ml. Current = 220 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.