A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours. Calculate the mass (in grams) of cadmium metal deposited. [Enter only numbers in the blank.]
4.2
three consecutive positive integers a,b and c are such that b2 = 4(a+c). find the value c
8.39g
To calculate the mass of cadmium metal deposited, we need to use the equation:
mass = (current × time × atomic mass) / (1 Faraday × number of electrons)
First, we need to determine the number of electrons involved in the reduction of Cd2+ ions to cadmium metal. Cadmium has a 2+ charge, and each Cd2+ ion gains two electrons to form cadmium metal, so the number of electrons (n) is 2.
Next, we need to find the atomic mass of cadmium (Cd) from the periodic table. The atomic mass of cadmium is approximately 112.41 g/mol.
The Faraday constant (F) represents the charge of one mole of electrons and is equal to 96,485 C/mol.
Now, let's substitute the given values into the equation:
current = 0.80 A
time = 2.5 hours = 2.5 × 3600 seconds (since 1 hour = 3600 seconds)
atomic mass (Cd) = 112.41 g/mol
number of electrons (n) = 2
Faraday constant (F) = 96,485 C/mol
mass = (0.80 A × 2.5 × 3600 s × 112.41 g/mol) / (1 mol e^- × 96,485 C)
Now, we can calculate the mass of cadmium deposited by substituting the values and performing the calculation:
mass = (0.80 A × 2.5 × 3600 s × 112.41 g/mol) / (1 × 96,485 C)
≈ (0.80 × 2.5 × 3600 × 112.41) / 96,485 g
≈ 621.28 / 96,485 g
Finally, we can simplify the result:
mass ≈ 0.00643 g
Therefore, approximately 0.00643 grams of cadmium metal will be deposited.
0.8 amp x 2.5 hours x (60 min/hr) x (60 s/min) = about 7200 Coulombs.
96,485 C will deposit one equivalent of Cd metal which is 112.41/2 = 56.2 g.
Cd deposited must be 56.2 g x (7200 C/96,485 C) = ?? g