Question

(i) Calculate the mass of silver deposited when a current of 4.6 A is passed through a solution of a silver salt for 90 minutes. [Ag = 108, 1 Faraday = 96,500 C]​

Answer 1

To calculate the mass of silver deposited, we need to use Faraday's laws of electrolysis. Faraday's first law states that the amount of a substance deposited during electrolysis is directly proportional to the amount of electricity passed through the electrolyte. The equation to calculate the mass of a substance deposited is:

Mass = (Current × Time × Atomic Mass) / (Electrical charge)

In this case, the current is given as 4.6 A and the time is given as 90 minutes. The atomic mass of silver is 108 g/mol, and the electrical charge is given as 1 Faraday = 96,500 C.

plug in the values into the equation:

Mass = (4.6 A × 90 minutes × 108 g/mol) / (96,500 C)

First, let's convert the time from minutes to seconds:

90 minutes = 90 × 60 seconds = 5400 seconds

Now, you can calculate the mass:

Mass = (4.6 A × 5400 seconds × 108 g/mol) / (96,500 C)

Mass = (111,024 g·s/A·mol) / (96,500 C)

Mass = 1.149 g

Therefore, the mass of silver deposited when a current of 4.6 A is passed through a solution of a silver salt for 90 minutes is approximately 1.149 grams.

:))))))))

Answer 2

0.0035 g

Chemistry Concept(s)

• Silver is a white, ductile metallic element, used for making mirrors, coins, ornaments, table utensils, photographic chemicals, conductors, etc. Symbol: Ag.
• Salt is a crystalline compounds, sodium chloride, NaCl, occurring as a mineral, a constituent of seawater, etc., and used for seasoning food, as a preservative, etc.

The mass of silver deposited can be calculated using Faraday's laws of electrolysis, which state that the amount of substance produced at an electrode is directly proportional to the amount of electrical charge passed through the electrode. The equation for calculating the mass of substance produced is:

⇒ mass = (current × time × atomic mass) / (charge × valence)

where:

• current is the current flowing through the cell in amperes (A)
• time is the time for which the current flows in seconds (s)
• atomic mass is the atomic mass of the substance being deposited in grams per mole (g/mol)
• charge is the charge on one electron in coulombs (C)
• valence is the number of electrons transferred in the reaction for the substance being deposited

In this case, the substance being deposited is silver (Ag), which has an atomic mass of 108 g/mol and a valence of 1 (as one electron is transferred in the reaction). The charge on one electron is 1.602 × 10^-19 C. One Faraday is equal to 96,500 C.

⇒ Substituting these values into the equation, we get:

• mass = (4.6 A × (90 minutes × 60 seconds/minute) × 108 g/mol) / (1.602 × 10^-19 C/electron × 1 electron × 96,500 C/Faraday)
• mass = 0.0035 g

Therefore, the mass of silver deposited is 0.0035 g.