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Answer: The amperage needed to complete the electrolysis in the given time is 9.08 A
Explanation:
We are given:
Moles of electron = 1 mole
According to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of particles.
We know that:
Charge on 1 electron = [tex]1.6\times 10^{-19}C[/tex]
Charge on 1 mole of electrons = [tex]1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C[/tex]
moles of calcium =[tex]\frac{\text {given mass}}{\text {Molar mass}}=\frac{99.47g}{40g/mol}=2.49moles[/tex]
[tex]Ca^{2+}+2e^-\rightarrow Ca[/tex]
[tex]2\times 96500=193000C[/tex] is required to deposit = 1 mole
Thus 1 mole is deposited by = 193000 C
2.49 moles will be deposited by =[tex]\frac{193000}{1}\times 2.49=480570C[/tex]
To calculate the time required, we use the equation:
[tex]I=\frac{q}{t}[/tex]
where,
I = current passed = ?
q = total charge = [tex]480570C[/tex]
t = time required = 14.7 hours =52920 s ( 1hour=3600s)
Putting values in above equation, we get:
[tex]I=\frac{480570C}{52920s}\\\\I=9.08A[/tex]
Hence, the amperage needed to complete the electrolysis in the given time is 9.08 A
The amount of current needed to complete the electrolysis in the given time is 9.08 A.
What information do we have?
Moles of electron = 1 mole
According to mole concept:
1 mole of an atom contains a number of particles.
We know that:
Charge on 1 electron = [tex]1.6*10^{-19} C[/tex]
Charge on 1 mole of electrons = [tex]1.6*10^{-19} C *6.022*10^{-23} =96500 C[/tex]
The moles of calcium = given mass / Molar mass
Moles of calcium = 2.49 moles
Thus 1 mole is deposited by = 193000 C
2.49 moles will be deposited by =193000 * 2.49 = 480570 C
Calculation for time required:
where,
I = current passed = ?
q = total charge = 480570 C
t = time required = 14.7 hours =52920 s ( 1hour=3600s)
On subsituting the values:
I= 480570 C / 52920 s = 9.08 A
Hence, the Current needed to complete the electrolysis in the given time is 9.08 A
Find more information about Current here:
brainly.com/question/24858512
