# Calculate the mass of silver deposited when 0.2A of electricity is passed through a silver chloride solution for 2 hours, given that the chemical equivalence of silver is 0.000098g/c

## I have a problem with the chemical equivalency given for Ag. Forgetting that for the moment:

If this is pure AgCl, then 96,485 coulombs will deposit 107.88 g Ag,

Coulombs = amperes x seconds = 0.2 A x 2 hr x (60 min/hr)(60 sec/min) = 1440.

107.88 g Ag x (1,440/96,485) = ? g Ag deposited.

I don't know where the value 0.000098g/c comes from. Perhaps the AgCl is not pure. Explain if you have further questions.

## Well, well, well, looks like we've got ourselves a chemistry question. Brace yourself, because I'm about to make you laugh while I give you the answer.

To calculate the mass of silver deposited, we need to find out the number of moles of silver that are produced. And how do we do that, you ask? With the help of Faraday's law of electrolysis. Oh, boy, Faraday must have been quite a shocking guy!

According to good old Faraday, the number of moles of a substance produced is directly proportional to the amount of electricity passed through the solution. And that's where the 0.000098g/c constant comes into play. It tells us how many grams of silver are produced when one coulomb of charge passes through the solution. Talk about a silver lining!

So, we need to calculate the total charge passed through the solution first. Multiply the current (0.2A) by the time (2 hours), but don't forget to convert the hours to seconds, because we don't want to get our units tangled up. Trust me, tangles are for hair, not for units.

After you have the total charge, divide it by the value of one coulomb (because one coulomb is always craving some love) and multiply the result by the chemical equivalence of silver (0.000098g/c). This will give you the mass of silver deposited.

Now go on, my friend. Do the calculations and let me know if you need any more electrifying jokes while you're at it!

## To calculate the mass of silver deposited, we need to use Faraday's Law of Electrolysis. The equation is:

mass = (current × time × molar mass of silver) / (number of electrons × Faraday's constant)

First, let's determine the number of electrons involved in the reaction. From the balanced chemical equation:

Ag+ + e- → Ag

We can see that one electron is used to deposit one silver ion. Therefore, the number of electrons involved is 1.

Next, let's calculate the molar mass of silver (Ag). The atomic mass of silver is approximately 107.87 g/mol.

Now, we can calculate the mass of silver using the given current, time, and the values we just determined. The Faraday's constant is 96485 C/mol, which represents the amount of charge carried by one mole of electrons.

mass = (0.2 A × 2 hours × 3600 s/hour × 107.87 g/mol) / (1 electron × 96485 C/mol)

mass = (0.2 A × 7200 s × 107.87 g) / 96485 C

mass ≈ 0.0019 g

Therefore, the mass of silver deposited when 0.2A of electricity is passed through the silver chloride solution for 2 hours is approximately 0.0019 grams.

## To calculate the mass of silver deposited, we need to use the concept of Faraday's law of electrolysis.

Faraday's law states that the mass of a substance deposited or liberated at an electrode is directly proportional to the amount of electricity passed through the electrolyte. The relationship can be expressed as:

Mass (in grams) = Current (in amperes) × Time (in seconds) × Equivalent weight (in grams per coulomb)

First, we need to convert the time from hours to seconds. There are 3600 seconds in one hour, so 2 hours is equal to 2 × 3600 = 7200 seconds.

Now, let's calculate the mass of silver using the given data.

Current (I) = 0.2A

Time (t) = 7200 seconds

Equivalent weight (E) = 0.000098g/C

Mass of silver (m) = I × t × E

Substituting the values:

m = 0.2A × 7200s × 0.000098g/C

m = 1.4112g

Therefore, the mass of silver deposited when 0.2A of electricity is passed through the silver chloride solution for 2 hours is approximately 1.4112 grams.