šŸ·ļø LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION ā†’
Log in
Chemistry
1
answer
0
watching
176
views
13 Dec 2019

  1. Nitrogen can be prepared by electrolysis of an aqueous nitratesolution

    1.

    False
    2.

    True

1 points

  1. What product(s) forms at the cathode in the electrolysis of anaqueous solution of NaF?

    1.

    Na
    2.

    O2 and H+
    3.

    F2
    4.

    H2 and OH-

Watch
1
answer
0
watching
176
views

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

Elin Hessel
Elin HesselLv2
17 Dec 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
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
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. What is the cell emf (Eocell) for electrolysis of molten nickel(II) iodide?




2. What reactions would take place at the anode and cathode duringelectrolysis of an
aqueous solution of nickel (II) iodide?









3. Use the Nernst Equation (Equation 7) to calculate Ecell at 25oCfor electrolysis of
aqueous sodium chloride if the concentration of chlorine in thebrine solution is 4.5
M and the partial pressure of Cl2 is 0.001 atmospheres.


4. Chlorine will spontaneously react with iodide to producechloride and iodine. What is Eo for this reaction.

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 Ć¢Ā†Ā’ 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) ƇĀ€ Zn2+(aq) (0.0420 M) ƇĀ€Ć‡Ā€ Tl3+(aq) (9.06ƃĀ—10-2 M), Tl+(aq) (0.0400 M) ƇĀ€ Pt(s).

Given: EƂĀ°(Zn2+/Zn) = - 0.763 V; EƂĀ°(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+

Write the half-reactions and the products for the reactions that occur in the electrolysis of a saturated solution of magnesium sulfate using inert electrodes. Choose at least one answer. should be 3-4 right answers a. 2Cl- ? 2Cl2(g) + 2e- (anode) b. 2H2O(l) ? O2(g) + 4H+(aq) + 4e- (anode) c. 2SO42-(aq) ? S2O82-(aq) + 2e- (anode) d. Ni(s) ? Ni2+(aq) + 2e- (anode) e. Ni2+(aq) + 2e- ? Ni(s) (cathode) f. Mg2+(aq) + 2e- ? Mg(s) (cathode) g. 2H2O (l) + 2e-? H2(g) + 2OH - (aq) (cathode) h. No net reaction. However, metal is transfer from the anode to the cathode. i. Cl2(g) j. H2(g) k. O2(g) l. Mg(s) m. Ni(s) n. S2O82-(aq) o. OH -(aq)

Weekly leaderboard

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