Three electrolytic cells containing solutions of CuNO3, Sn(NO3)2, and Fe(NO3)3, respectively, are connected in series. A current of 2.2 A is passed through the cells until 3.10 g of copper has been deposited in the cell.

(a) What masses of tin and iron are deposited?

found electron to mole ratio for each but still cant figure out what to do. thx

96,485 coulombs will deposit 1 equivalent weight of a metal. For Cu, that is

95,485C will deposit 63.546/2= 31.77 g. The deposit was 3.10 g and that is 3.10/31.77 = 0.0976 C that flowed through the cells.
1 equivalent weight Sn = 118.71/2 = ??
1 equivalent weight Fe = 55.85/3 = 18.61
For Fe the deposit is 18.61 x 0.0976 = 1.82 g. Do the same for Sn.

To determine the masses of tin and iron deposited, we can start by calculating the number of moles of copper that was deposited in the first cell.

Step 1: Calculate the moles of copper deposited
To do this, we need to use the molar mass of copper (Cu). The molar mass of copper can be found on the periodic table and is 63.55 g/mol.

molar mass of Cu = 63.55 g/mol

To find the number of moles (n) of copper deposited, we can use the formula:

n = mass / molar mass

Given that the mass of copper deposited is 3.10 g, we can substitute these values into the formula:

n(Cu) = 3.10 g / 63.55 g/mol

n(Cu) ≈ 0.0488 mol

Step 2: Determine the mole ratio of copper to tin and iron
Now, we need to use the mole ratios from the balanced chemical equations for the electrolysis reactions. The balanced equations for the reactions are as follows:

Cu²⁺ + 2e⁻ → Cu (copper deposition)
Sn²⁺ + 2e⁻ → Sn (tin deposition)
Fe³⁺ + 3e⁻ → Fe (iron deposition)

From these equations, we can see that the mole ratio of copper to tin is 1:1, and the mole ratio of copper to iron is 2:3.

Step 3: Calculate the moles of tin and iron deposited
Using the mole ratio, we can determine the moles of tin and iron deposited by multiplying the moles of copper deposited by the corresponding mole ratios.

Moles of tin deposited = n(Cu) × mole ratio(Cu to Sn)
Moles of iron deposited = n(Cu) × mole ratio(Cu to Fe)

Substituting the values we have:

Moles of tin deposited = 0.0488 mol × 1 mol Sn / 1 mol Cu
Moles of iron deposited = 0.0488 mol × 2 mol Fe / 3 mol Cu

Step 4: Convert moles to mass
To find the masses of tin and iron deposited, we need to multiply the corresponding moles by their respective molar masses (found on the periodic table).

Mass of tin deposited = Moles of tin deposited × molar mass of Sn
Mass of iron deposited = Moles of iron deposited × molar mass of Fe

Given that the molar masses of tin (Sn) and iron (Fe) are 118.71 g/mol and 55.85 g/mol, respectively, we can calculate the masses:

Mass of tin deposited ≈ Moles of tin deposited × 118.71 g/mol
Mass of iron deposited ≈ Moles of iron deposited × 55.85 g/mol

Calculating these values will give you the masses of tin and iron deposited in the electrolytic cells.

To determine the masses of tin and iron deposited, we need to employ Faraday's law of electrolysis. According to this law, the amount of substance deposited or liberated during an electrolysis process is directly proportional to the quantity of electricity passed through the electrolyte.

The key idea is to use the relationship between current (I), time (t), charge (Q), and Faraday's constant (F):

Q = I * t

where:
Q is the charge passed in coulombs (C),
I is the current in amperes (A), and
t is the time in seconds (s).

The charge passed (Q) is related to the number of moles of substance deposited (n) by the equation:

n = Q / (z * F)

where:
z is the number of electrons exchanged per mole of substance, and
F is Faraday's constant (96,485 C/mol).

First, we need to find the number of moles of copper deposited, as this information is given in the question. The molar mass of copper (Cu) is approximately 63.55 g/mol.

n(Cu) = mass(Cu) / molar mass(Cu)
n(Cu) = 3.10 g / 63.55 g/mol

Now, let's calculate the charge passed for copper using Faraday's law:

Q(Cu) = n(Cu) * z(Cu) * F

The number of electrons exchanged for copper (Cu) can be determined from its oxidation state. In this case, each copper atom gains two electrons during reduction, resulting in z(Cu) = 2.

Now, let's determine the charge passed for copper using the given current:

Q(Cu) = I * t

We can substitute this value into the equation above.

Next, we can calculate the number of moles of tin deposited using Faraday's law:

n(Sn) = Q(Sn) / (z(Sn) * F)

Similarly, we find the number of moles of iron deposited using Faraday's law:

n(Fe) = Q(Fe) / (z(Fe) * F)

For tin, the number of electrons exchanged per mole of substance (z value) can be determined from its oxidation state, and the same for iron.

Finally, we can calculate the masses of tin and iron deposited using their moles and molar masses:

mass(Sn) = n(Sn) * molar mass(Sn)
mass(Fe) = n(Fe) * molar mass(Fe)

After obtaining the number of moles for tin and iron, multiply them by their respective molar masses to find their masses deposited.

Note: It's essential to consider the correct signs of charges when setting up the equations, based on whether the substance is being oxidized or reduced during the electrolysis process.