Question

A Cr3+(aq) solution is electrolyzed, using a current of 7.80 A . 1. What mass of...

A Cr3+(aq) solution is electrolyzed, using a current of 7.80 A .

1. What mass of Cr(s) is plated out after 1.50 days?


2.What amperage is required to plate out 0.200 mol Cr from a Cr3+ solution in a period of 7.00 h ?

Homework Answers

Answer #1

1) 7.80A = 7.80 Coulomb per second

Coulomb in 1.50 days = 129600 × 7.80 = 1010880C

No of mole of electron = 1010880/96485 = 10.477

No of mole of electron required to deposit 1mol of Cr = 3

No of mole of Cr3+ deposited = 10.477/3= 3.4923

molar mass of Cr = 51.996g/mol

Mass of Cr plated = 51.996g/mol × 3.4923mol = 181.59g

2) mole of Cr plated out = 0.200mol

mole of electron required = 3×0.2 = 0.6mol

Coulombs required = 0.6 × 96485 = 57891C

plating period = 7 hours = 25200seconds

Amperage required = 57891/25200=2.297A

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A Cr3+(aq) solution is electrolyzed, using a current of 7.40 A . What mass of Cr(s)...
A Cr3+(aq) solution is electrolyzed, using a current of 7.40 A . What mass of Cr(s) is plated out after 2.50 days? What amperage is required to plate out 0.210 mol Cr from a Cr3+ solution in a period of 8.40 h ?
A Cr3+(aq) solution is electrolyzed, using a current of 6.40 A . Part A What mass...
A Cr3+(aq) solution is electrolyzed, using a current of 6.40 A . Part A What mass of Cr(s) is plated out after 2.50 days? Part B What amperage is required to plate out 0.270 mol Cr from a Cr3+ solution in a period of 8.30 h ?
What mass of Cr(s) (in g) may be electrodeposited from application of a 0.436 A current...
What mass of Cr(s) (in g) may be electrodeposited from application of a 0.436 A current to a solution of Cr3+(aq) over 3.57 min?
Cadmium metal is added to 0.350 L of an aqueous solution in which [Cr3+]=1.00M. 2Cr3+(aq)+Cd(s)⇌2Cr2+(aq)+Cd2+(aq)KC=0.288 What...
Cadmium metal is added to 0.350 L of an aqueous solution in which [Cr3+]=1.00M. 2Cr3+(aq)+Cd(s)⇌2Cr2+(aq)+Cd2+(aq)KC=0.288 What is the concentration of Cr2+ at equilibrium? What is the concentration of Cd2+ at equilibrium? What is the concentration of Cr3+ at equilibrium? What is the minimum mass of cadmium metal required to establish this equilibrium?
A solution of AgNO3 is electrolyzed by passing 144 A of current for 102 min. What...
A solution of AgNO3 is electrolyzed by passing 144 A of current for 102 min. What mass of silver plates out? Want to see how it is worked.
Silver can be plated out of a solution containing Ag+ according to the half-reaction Ag+(aq)+e−→Ag(s) How...
Silver can be plated out of a solution containing Ag+ according to the half-reaction Ag+(aq)+e−→Ag(s) How much time (in minutes) does it take to plate 12 g of silver using a current of 4.4 A ?
Silver can be plated out of a solution containing Ag+ according to the half-reaction Ag+(aq)+e−→Ag(s) How...
Silver can be plated out of a solution containing Ag+ according to the half-reaction Ag+(aq)+e−→Ag(s) How much time (in minutes) does it take to plate 14 g of silver using a current of 3.3 A ?
An aqueous ScF3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the...
An aqueous ScF3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C F2(g) + 2 e- ---------> 2 F-(aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e- --------> 6 H2O(l) 1.229 2 H2O(l) + 2 e- -------> H2(g) + 2 OH-(aq) -0.828 Sc3+(aq) + 3 e- ---------> Sc(s) -2.080 Half-reaction at anode:...
You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.200...
You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.200 M HCl(aq) solution is needed to precipitate the silver ions from 13.0 mL of a 0.180 M AgNO3 solution
1. The standard reduction potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Using...
1. The standard reduction potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Using Appendix E in the textbook, which of the following substances is capable of reducing Eu3+(aq) to Eu2+(aq) under standard conditions? a. Al B. Co C. H2O D. N2H5 E. H2C2O4 2. How many minutes will it take to plate out 4.56 g of Ni metal from a solution of Ni2+ using a current of 40.5 amps in an electrolytic cell? 3. Using the standard...