31. An unknown metal M is reduced by electrolysis from a solution of M(NO3)3. It took 74.1 s for a current of 2.00 A to plate out 0.107 g of the metal. Identify the metal.
31. An unknown metal M is reduced by electrolysis from a solution of M(NO3)3. It took 74.1 s for a current of 2.00 A to plate out 0.107 g of the metal. Identify the metal.
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter24: Coulometry
Section: Chapter Questions
Problem 24.4QAP: Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose...
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PLESE ANSWER QUESIN NUM 31
![30.
31.
32.
33.
(d)
Cl + e
Cl²-
What volumes of H₂ (g) and O₂ (g) at STP are produced from the electrolysis of
water by a current of 2.50 A in 15.0 minutes?
→
An unknown metal M is reduced by electrolysis from a solution of M(NO3)3. It
took 74.1 s for a current of 2.00 A to plate out 0.107 g of the metal. Identify the
metal.
An aqueous solution contains a mixture of cations at the following concentrations.
[Cd²+] =
= 1.0 M
[Fe²+] = 0.10 M
[Ni²+] = 1.0 x 10-6 M
In which order will these metal cations be reduced if an applied voltage to the
solution is gradually increased?
Consider the electrolysis of a solution that is 1.0 x 10³ M in Ag₂SO4 and
1.0 x 10¹¹ M in ZnSO4 with pH = 2.000.
(a)
(b)
Calculate the minimum voltage needed to plate silver metal at the cathode.
Will it be possible to plate zinc metal at the cathode once the concentration
of Agt has been reduced to a sufficiently low value?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F42f22682-25cf-4dd2-8ed0-9de681e62a40%2Fbeddc368-6844-4f35-a98e-98ccf5503d93%2Fpkypwsj_processed.png&w=3840&q=75)
Transcribed Image Text:30.
31.
32.
33.
(d)
Cl + e
Cl²-
What volumes of H₂ (g) and O₂ (g) at STP are produced from the electrolysis of
water by a current of 2.50 A in 15.0 minutes?
→
An unknown metal M is reduced by electrolysis from a solution of M(NO3)3. It
took 74.1 s for a current of 2.00 A to plate out 0.107 g of the metal. Identify the
metal.
An aqueous solution contains a mixture of cations at the following concentrations.
[Cd²+] =
= 1.0 M
[Fe²+] = 0.10 M
[Ni²+] = 1.0 x 10-6 M
In which order will these metal cations be reduced if an applied voltage to the
solution is gradually increased?
Consider the electrolysis of a solution that is 1.0 x 10³ M in Ag₂SO4 and
1.0 x 10¹¹ M in ZnSO4 with pH = 2.000.
(a)
(b)
Calculate the minimum voltage needed to plate silver metal at the cathode.
Will it be possible to plate zinc metal at the cathode once the concentration
of Agt has been reduced to a sufficiently low value?
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