Question

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 ?


Homework Answers

Answer #1

If you have any query please comment

If you satisfied with the solution please rate it thanks

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 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 ?
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 ?
Part A What mass of Cu(s) is electroplated by running 18.0 A of current through a...
Part A What mass of Cu(s) is electroplated by running 18.0 A of current through a Cu2+(aq) solution for 4.00 h? Express your answer to three significant figures and include the appropriate units. Part B How many minutes will it take to electroplate 37.1 g of gold by running 5.00 A of current through a solution of Au+(aq)? Express your answer to three significant figures and include the appropriate units.
what mass of Ru (ruthenium) is produced during the electrolysis of a solution Ru(NO3)2 with a...
what mass of Ru (ruthenium) is produced during the electrolysis of a solution Ru(NO3)2 with a 2.50 A current applied for 22.0 minutes? The cell potential E is 0.97V and Ecell is 1.21V in the following voltaic cell: Ni(s)|Ni2+(aq)(0.88M)||NO3-(aq)(1.45M),H+(aq)(??M)|NO(g)(0.75atm)|Pt(s) what is the pH in the cell?
Part 1: What is the concentration of your NaOH(aq) solution? 1.00×10-1 M NaOH Ok. Part 2:...
Part 1: What is the concentration of your NaOH(aq) solution? 1.00×10-1 M NaOH Ok. Part 2: You will then make a Kool-Aid solution by dissolving the powder in an entire packet of lemon-lime Kool-Aid in 250.00 mL solution.  You find the powder in a packet of lemon-lime Kool-Aid has a mass of 3.654 g. In Part 2 of the lab you titrate 5.00 mL of the lemon-lime Kool-Aid (with 5 drops of thymol blue indicator) with your NaOH(aq) solution. The titration...