Respuesta :
Answer:
16.36A
Explanation:
We'll begin by writing a balanced dissociation equation of aqueous Cr2(SO4)3. This is illustrated below:
Cr2(SO4)3 —> 2Cr^3+ 3(SO4)^2-
From the above, we can see that Cr is trivalent.
Next, let us determine the number of faraday needed to deposit metallic Cr. This is illustrated below:
Cr^3+ 3e- —> Cr
From the above equation, 3 faradays are needed to deposit metallic Cr
1 faraday = 96500C
Therefore, 3 faraday = 3 x 96500C = 289500C.
Molar Mass of Cr = 52g/mol
Now let us determine the quantity of electricity needed for 2.68g of Cr metal
This is shown below:
52g of Cr required 289500C.
Therefore, 2.68g of Cr will require = (2.68 x 289500)/52 = 14920.38C
Now, with this quantity of electricity (i.e 14920.38C), we can easily calculate the current needed for the process. This is illustrated below:
Q (quantity of electricity) = 14920.38C
t (time) = 15.2mins = 15.2 x 60 = 912secs
I (current) =?
Apply the equation Q = It
Q = It
14920.38 = I x 912
Divide both side by 912
I = 14920.38/912
I = 16.36A
Therefore, a current of 16.36A is needed for the process.
The current needed is 16.36 A. The quantity of electricity (i.e 14920.38C), we can easily calculate the current needed for the process.
Balanced dissociation equation:
[tex]Cr_2(SO_4)_3 ---- > 2Cr^{3+}+ 3SO_4^{2-}[/tex]
The number of faradays needed to deposit metallic Cr. This is illustrated below:
[tex]Cr^{3+}+ 3e^- ---- > Cr[/tex]
Given:
3 faradays are needed to deposit metallic Cr
1 faraday = 96500C
Therefore, 3 faraday = 3 * 96500C = 289500C.
Molar Mass of Cr = 52g/mol
52g of Cr required 289500C.
Therefore, 2.68g of Cr will require = (2.68 * 289500)/52 = 14920.38C
Now, with this quantity of electricity (i.e 14920.38C), we can easily calculate the current needed for the process. This is illustrated below:
Q (quantity of electricity) = 14920.38C
t (time) = 15.2mins = 15.2 x 60 = 912secs
To find:
I (current) =?
Apply the equation,
Q = It
14920.38 = I * 912
I = 14920.38/912
I = 16.36A
Therefore, a current of 16.36A is needed for the process.
Find more information Dissociation equation here:
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