Question

A current of 3.53 A is passed through a Ni(NO3)2 solution for 1.70 hours. How much nickel is plated out of the solution?

Answer #1

Firstly we need to get Coulomb from Ampere as:

3.53 A x 1.70 hours x (3600 sec / 1 hour) = **21603.6
C**

Now,

To get moles of electron we would solve as:

21603.6 C / 96485 Cmol^{-1} electron = **0.224
moles electron**

**The equation will be as: Ni ^{2+} +
2e^{-} ---> Ni**

In order to get moles , we need to divide the moles of electrons
by 2 (since Ni^{2+} needed 2 electrons per ion to
neutralize and plate out as we can see from the equation)

So, 0.224 moles electron / 2 electron = **0.112 mol
Ni**

Again, we know molar mass of Nickel (NI) is 58.6934 g/mol

Thus, 0.112 mol Ni x( 58.6934 g Ni / 1 mol Ni) = 6.57 g Ni

**Hence, amount of nickel plated out of the solution =
6.57 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
1.20 hours. How much tin is plated out of the solution?

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

A current of 5.22 A5.22 A is passed through a Sn(NO3)2Sn(NO3)2
solution for 1.60 h1.60 h. How much tin is plated out of the
solution?

A current of 5.94A is passed through a
Cu(NO3)2 solution. How long (in hours)would
this current have to be applied to plate out 6.30g of
copper?

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
9.00 g of tin?

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
5.20 g of chromium?

A current of 5.02 A is passed through a Sn(NO3)2 solution. How
long (in hours) would this current have to be applied to plate out
6.30 g of tin?

A current of 3.56 A is passed through a Cu(NO3)2 solution. How
long (in hours) would this current have to be applied to plate out
8.60 g of copper?
Can someone list out the steps to solving this problem, would
help a lot.

How many grams of nickel metal are plated out when a constant
current of 15.0 A is passed through aqueous NiCl2 for
60.0 minutes?
Stuff you need: Ni+2 needs two moles of e-
to form 1 mole of Ni metal; 1 A = 1 Coulomb/sec; 1 mol e- = 96,485
C.

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