Log in
Chemistry
1
answer
0
watching
183
views
18 Nov 2019

Calculate the time required for a constant current of 0.898 A to deposit 0.354 g of Tl(III) as Tl(s) on a cathode.

s=?

Calculate the mass of Tl(I) that can be deposited as Tl2O3(s) on an anode at a constant current of 0.898 A over the same amount of time as calculated above.

g=?

Watch
1
answer
0
watching
183
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Nestor Rutherford
Nestor RutherfordLv2
18 Nov 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

1) A constant current of 0.800 A is run through the electrolytic cell in order to produce oxygen (gas) at the anode:

2 H2O → O2(g) + 4 e- + 4 H+

The amount (in grams) of O2 obtained after 15.2 min of electrolysis is [X] g

2) Electrolysis of a solution of Tl3+ produces deposition of elemental thallium, Tl, at the cathode. The time (in min.) needed for a constant current of 1.20 A to deposit 0.500 g of Tl(s) is [X] min.

3) An electrochemical cell is described by the following line notation:

Zn(s) ǀ Zn2+(aq) (0.0420 M) ǀǀ Tl3+(aq) (9.06×10-2 M), Tl+(aq) (0.0400 M) ǀ Pt(s).

Given: E°(Zn2+/Zn) = - 0.763 V; E°(Tl3+/Tl+) = + 1.25 V.

The potential on the cathode half-cell, E+ = V; the potential on the anode half-cell, E- = V; and the overall cell potential, Ecell = V.

4) Consider electrolysis of molten copper bromide, CuBr2. What is the product of this process obtained (a) at the cathode? (b) at the anode?

1. a) Cathode: Cu(s);
(b) Anode: Br2(l)

2. (a) Cathode: Br2(l);

(b) Anode: Cu(s)

3. (a) Cathode: Cu2+;

(b) Anode: Br-

4. (a) Cathode: Br-;

(b) Anode: Cu2+

5. (a) Cathode: Cu(s);

(b) Anode: O2(g)

6. (a) Cathode: H2(g);

(b) Anode: Cu2+

Silver is deposited from a plating solution of Ag+ , at a constant current of 0.850 Amp for 1 hour 32 minutes and 15 seconds.

The platinum cathode had initial mass 19.3418 g, and final mass 21.0045 g.

(a) What mass of Ag was deposited? How many moles is this? How many coulombs were required to deposit this amount?

(b) Assuming the only other reaction occurring at the cathode was:

2H+ + 2 e- --> H2(g), calculate the moles of H2 produced.

Be sure to answer all parts. When an aqueous solution containing gold (III) salt is electrolyzed, metallic gold is deposited at the cathode, and oxygen gas is generated at the anode. (a) If 8.75 g of Au is deposited at the cathode, calculate the volume of O2 generated at 23°C and 770 mmHg. L (b) What is the current used if the electrolytic process took 4.10 h? A

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in