Question

A current of 5.66 A is passed through a Cr(NO3)2 solution for 1.20 hours. How much chromium is plated out of the solution?

____g

Answer #1

the electrolysis expression is:

Cr2+ + 2e- ------> Cr

1 mol of Cr requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Cr requires 192970 C

let us calculate the charge passed:

t = 1.2 hr = 1.2*3600 s = 4320 s

time, t = 4320s

Q = I*t

= 5.66A * 4320s

= 24451.2 C

mol of Cr plated = 24451.2/192970 = 0.12671 mol

Molar mass of Cr = 52 g/mol

mass of Cr = number of mol * molar mass

= 0.12671 * 52

= 6.59 g

Answer = 6.59 g

A current of 4.08 A is passed through a Cr(NO3)2 solution for
1.70 hours. How much chromium is plated out of the solution?
Please include steps so I understand. Thank you.

A current of 4.69 A is passed through a Sn(NO3)2 solution for
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A current of 4.24 A is passed through a Cr(NO3)2 solution. How
long (in hours) would this current have to be applied to plate out
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A current of 3.53 A is passed through a Ni(NO3)2 solution for
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A current of 5.22 A5.22 A is passed through a Sn(NO3)2Sn(NO3)2
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A current of 5.94A is passed through a
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A current of 3.01 A is passed through a Sn(NO3)2 solution. How
long (in hours) would this current have to be applied to plate out
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A current of 5.02 A is passed through a Sn(NO3)2 solution. How
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A solution is made by dissolving 23.2g of Chromium (II) nitrate,
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Cr(NO3)2= mol/L
Cr^2+= mol/L
NO3- = mol/L

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