CuSO4 Solution

%% CuSO4 Solution
% Determines how much copper is deposited on the cell
% Notes and clarifications are at the bottom of the code

% Constants
massCu = 63.5;                     % [g/mol] The atomic mass of copper
eCharge = 1.6*10^-19;              % [C] The charge of an electron
Na = 6.02*10^23;                   % [1/mol] Avogadro's constant

% Inputs and Variables
I = input('The current running through the solution in Amps\n');
deltat = input('The duration in hours\n') * 3600;

% Outputs and Equations
Q = I * deltat;                 % [C] The total charge
NumOfE = Q/eCharge;             % [electrons] The number of electrons
NumOfCu = NumOfE/2;             % [Cu atoms] The number of Copper atoms
n = NumOfCu/Na;                 % [mol] The number of Cu Moles
depoMass = n * massCu;          % [g] Deposited Copper mass
fprintf('The copper deposited is %e g', depoMass);

%{

There are a lot more notes than usual so please take the time to read

Under the assumption that an electric current runs thorugh an electrolytic
    cell containing copper-sulfate solution.
Notice that for this code the user input for time is in hours. However, the
    variable deltat is in seconds. To change this edit line 12.
The atomic mass of copper is not technically a constant but it is the
    average mass of copper and will be used as a constant for this code.
The reason the number of electrons is divided by 2 in line 17 to equal the
    number of Cu atoms is because 2 electrons are required to neutralize a
    Cu2+ ion
The units for Avogadro's number is usually mol. However in this code the
    degree power is 23 not -23, so the units are 1/mol.
This code can be changed for any electrolytic solution by changing the
    atomic mass in line 6, the number of electrons needed to neutralize the
    ion in line 17, and the name of variables and fprintf line.
%}