Calculate the mass of silver deposited when 0.4A of electricity is passed through a silver chloride solution for 2 hours , given that the chemical equivalent of silver is 0.000098g/c
To calculate the mass of silver deposited, we can use Faraday's law of electrolysis. The formula is as follows:
Mass (in grams) = Current (in amperes) × Time (in seconds) × Equivalent mass (in grams per coulomb)
In this case, we need to convert the time from hours to seconds since the formula requires the time in seconds.
1 hour = 60 minutes
1 minute = 60 seconds
So, 2 hours is equal to 2 × 60 × 60 = 7200 seconds.
Now, we can calculate the mass of silver deposited using the given information:
Mass = 0.4 A × 7200 s × 0.000098 g/C
Mass = 28.224 g
Therefore, the mass of silver deposited when 0.4 A of electricity is passed through a silver chloride solution for 2 hours is 28.224 grams.
I believe you have made a typo or the problem has the wrong information. According to my information the chemical equivalency of Ag is 1.118 mg Ag/C. But forget that for the moment and solve the problem using coulomgs like this.
coulombs = amperes x seconds
C = 0.4 x 2 hrs x (60 min/hr) x (60 sec/min) = 2880
96,485 coulombs will deposit 107.9 g Ag so
107.9 x (2,880/96,485) = 3.22 g Ag
Or from my number above of 1.118 mg Ag/C it will be
1.118 mg Ag/C x 2,880 C = 3219.8 which rounds to 3220 mg or 3.22 g so the answer is 3.22 g Ag will be deposited. I don't know where the 0.000098 g/c comes from.
To calculate the mass of silver deposited when a certain amount of electricity is passed through a solution, we need to use Faraday's law of electrolysis. According to this law, the mass of a substance produced during electrolysis is directly proportional to the amount of electricity passed through the solution.
Let's break down the steps to calculate the mass of silver deposited:
1. Determine the total charge passed through the solution:
Charge (Q) = Current (I) × Time (t)
Here, the current is given as 0.4A (amperes), and the time is given as 2 hours. However, to use this information accurately, we need to convert the time to seconds:
Time (t) = 2 hours × 60 minutes/hour × 60 seconds/minute
Now we can calculate the charge:
Q = 0.4A × 2 × 60 × 60 seconds
2. Calculate the number of moles of electrons (n):
To do this, we divide the total charge (Q) by Faraday's constant (F), which is equal to 96,485 Coulombs (C) per mole of electrons:
n = Q / F
Since we know that 1 Coulomb (C) = 1 Ampere-second (A·s), we can substitute the value of F:
n = Q / (96,485 C/mol)
3. Calculate the number of moles of silver (Ag):
This can be done by multiplying the number of moles of electrons (n) by the stoichiometric ratio between the electrons and silver ions involved in the reaction. For silver, the chemical equation shows that the stoichiometry is 1 mole of electrons per 1 mole of silver:
moles of silver (Ag) = n
4. Calculate the mass of silver (Ag):
Finally, multiply the number of moles of silver (Ag) by the molar mass of silver. The molar mass of silver is given as 0.000098g:
mass of silver (Ag) = moles of silver (Ag) × molar mass of silver
By following these steps, you can calculate the mass of silver deposited using the given values.