Solid, metallic chromium can be electroplated from acidic aqueous solutions containing dichromate ions (Cr20,2-). What would be the minimum amount of time (in minutes) needed to plate out 126.7 g of chromium metal is electroplated from such a solution using a current of 69 A? (Molar mass: Cr = 51.9961 g/mol) Cr20,2 (aq) + 2e --> Cr(s) Instructions: ***Do not enter the unit. Just enter the numerical value (be sure to include "-" negative sign if your value is negative. Do not include "+" positive sign if your answer is positive. ***Enter your value to the nearest hundredth (or 0.01). If your enter 1.50. Do not worry if Canvas rounds your answer to 1.5. Canvas will treat 1.5 and 1.50 as being the same.

Q: 6b. How long does it take to deposit a coating of gold 1.00 picometers thick on a disk-shaped…

A:

Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl2(g) -> 2 Ag+(aq) + 2 Cl2-…

A: Nernst equation is used to  calculate cell potential or  cell voltage as follows

Q: Ⓒ Macmillan Learning Calculate the cell potential for the reaction as written at 25.00 °C, given…

A: Given

Q: A galvanic cell is constructed in which the overall reaction is: Br2(1) + H2(9) → 2Brag) + 2H+…

A:

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

A: Given-> Concentration of VO2+ = 3.63 M Concentration of H+ = 1.38 M Concentration of VO2+ = 0.607…

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

A:

Q: An electrochemical bromate/bromide 3 Cu(s) + BrO3(aq) + 6 H*(aq) → 3 Cu2+ (aq) + Br¯(aq) + 3 H₂O(l)…

A:

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: Here we first need to determine the half-cell reactions so that we can find out the no of electrons…

Q: - hours wor

A:

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: Use Nerenst  equation and standard  data E (cathode) =0.53 V E (Anode) =- 0.15 V

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: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Given-> [Cr2+] = 0.790 M [Fe2+] = 0.0190 M T = 25°C

Q: An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of…

A: Electrolysis is spitting of chemical decomposition of ionic substances due to passage of electric…

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

A:

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: (a) Write the anode and cathode reactions and the overall reaction occurring in a lead storage…

A:

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

A:

Q: hromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Cr(s)+Fe+2 (aq )<==>  Cr+2 (aq)+Fe(s) [Cr+2] = 0.768 M [Fe+2] = 0.0170 M

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

A:

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: A galvanic was using the following electrode reactions. Co(s) + 3 en (aq) → [Co(en)3]²+ (aq) + 2 e¯…

A: We have to find formation constant.

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

A: We can use Nerst Equation to solved the above problem.

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Answer:- This question is answered by using the simple concept of calculation of cell potential…

Q: 32. What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for…

A: Given that,time, t = 244.7 min = 244.7 x 60 sec = 14682 seccurrent, i = 13.6 A F = 96485…

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: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction. Ti(s)+Cu2+(aq)↽−−⇀…

A: Given Data:

Q: current of 70.9 A is applied to a 0.123 mol L-1 solution of Pt2+ how many seconds would it take to…

A: Here we know nF of charge is required to produce 1 mole of Pt (s) as the products. So we do the…

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.35 M), Cr3+ (2.0 M) || Co2+ (0.24 M) | Co…

A: The cell reaction is, The value of K is 2.79 ✕ 107 The reaction taking place at cathode is, The…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Cr(s)+Fe+2 (aq )<==>  Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.807 M and…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Current = 5 A Voltage = 4.5 V Time = ? Volume = 215 mL = 0.215 L Molarity = 1.19 M

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co2+ (0.20 M) | Co…

A:

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M…

A: Given data :  Cr(s) + Fe2+ (aq) ==> Cr2+(aq) + Fe(s)  From table :  E(Fe2+/Fe) = -0.44 V…

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

A:

Q: Consider this galvanic cell at 298 K:                 2 Cr(s)  +  3 Ni2+(aq)      2 Cr3+(aq)  +…

A:

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A:

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: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Recall the given reaction         Zns + Sn2+aq → Zn2+aq + SnsAccording to Nernst equation Cell…

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

A:

Q: A galvanic cell is constructed using the following half-reactions at 298 K. Given Kf = 1.0 x 10^8…

A: Given formation constant for MX42+(aq) , Kf = 1.0*108  Since Kf >> 1, formation of MX42+(aq)…

Q: Given: Zn2+(aq) + 2e–  Zn(s); E° = –0.76 V Cu2+(aq) + 2e–  Cu(s); E° = 0.34 V What is the cell…

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.