Respuesta :
Explanation:
(a) It is given that for [tex]Al^{3+}[/tex] value of current is 1.234 A.
Hence, total charge Q = [tex]\frac{3 mol e^{-} \times 96485 C}{1.00 mol e^{-}}[/tex]
= 289455 C
Now, we will calculate the time as follows.
t = [tex]\frac{Q}{I}[/tex]
= [tex]\frac{289455 C}{1.234 C/s}[/tex]
= 234566.4506 s
or, = [tex]\frac{234566.4506 s}{3600 s} \times 1 hr[/tex]
= 65.16 hr
(b) It is given that for [tex]Ca^2+[/tex], value of current is 22.2 A.
Hence, its total charge Q = [tex]\frac{2 mol e^- \times 96485 C}{1.00 mol e^-}[/tex]
= 192970 C
Now, we will calculate the time as follows.
t = [tex]\frac{Q}{I}[/tex]
= [tex]\frac{192970 C}{22.2 C/s}[/tex]
= 8692.34 s
or, = 2.4 hr
(c) It is given that for [tex]Cr^5+[/tex], value of current is 37.45 A.
Hence, the total charge Q = [tex]\frac{5 mol e^{-} \times 96485 C}{1.00 mol e^{-}}[/tex]
= 482425 C
Now, we will calculate the time as follows.
t = \frac{Q}{I}[/tex]
= \frac{482425 C}{37.45 C/s}[/tex]
= 12881.8 s
or, = 3.6 hr
(d) It is given that for [tex]Au^{3+}[/tex], value of current is 3.57 A.
Hence, the total charge Q = [tex]\frac{3 mol e^{-} \times 96485 C}{1.00 mol e^{-}}[/tex]
= 289455 C
Now, we will calculate the time as follows.
t = [tex]\frac{Q}{I}[/tex]
= [tex]\frac{289455 C}{3.57 C/s}[/tex]
= 81079.83 s
= 22.5 hr
Based on the charge on the ions and the current suppied, the time taken to discharge mole of each of the ions are:
- 65.17 hours for 1 mole of Al3+
- 2.41 hours for 1 mole of Ca2+
- 3.58 hours for 1 mole of Cr5+
- 22.52 hours for 1 mole of Au3+
What is the relationship between ionic charge and moles of substance discharged?
The moles of a substance discharge is inversely related to the charge on the ion and directly proportional to the quantity of charge applied.
- Quantity of charge = current × time in seconds
Q = It
Time = Q/I
1 Faraday = 96500 C
Al3+ will require 3 Faradays of charge
3 Faradays = 289500
T = 289500/1.234 seconds × 1 hr/3600 seconds
T = 65.17 hours
Ca2+ will require 2 Faradays of charge
2 Faradays = 193000
T = 19300/22.2 seconds × 1 hr/3600 seconds
T = 2.41 hours
Cr5+ will require 6 Faradays of charge
5 Faradays = 482500
T = 482500/37.45 seconds × 1 hr/3600 seconds
T = 3.58 hours
Au3+ will require 3 Faradays of charge
3 Faradays = 289500
T = 289500/3.57 seconds × 1 hr/3600 seconds
T = 22.52 hours
Therefore, the time taken to discharge 1 mole of each of the ions are:
- 65.17 hours for 1 mole of Al3+
- 2.41 hours for 1 mole of Ca2+
- 3.58 hours for 1 mole of Cr5+
- 22.52 hours for 1 mole of Au3+
Learn more about quantity of charge and moles at: https://brainly.com/question/18752494
