A current of 5A was passed through a solution of nickel (1)(1))salt.find the time taken for 6g of nickel to be deposited
Oh my. How many electrons?
Nickel is 58.7 grams per mole or 6*10^23 atoms which here is 6*10^23 electros
so
6 g * 6.022*10^23 electrons/58.7 g
= .6155 * 10^23 electrons
1.602*10^-19 coulomb/electron
so the product is
.986 * 10^4 Coulombs
a coulomb is an amp second
so
.986*10^4 = 5 t
t = .197 * 10^4 seconds
= 1970 seconds
= about 33 minutes
check my algebra !
Excellent
how did u get the answers
To find the time taken for 6g of nickel to be deposited, we'll need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the solution.
First, we need to convert the mass of nickel (6g) to moles. The molar mass of nickel is 58.69 g/mol, so:
Number of moles of nickel = mass of nickel / molar mass of nickel
Number of moles of nickel = 6g / 58.69 g/mol ≈ 0.102 moles
Since the stoichiometry of the reaction tells us that one mole of nickel (Ni) requires two moles of electrons (2e-) to be deposited, we can determine the total charge required using Faraday's constant (F), which is 96,485 Coulombs per mole of electrons.
Total charge required = number of moles of electrons × Faraday's constant
Total charge required = 0.102 moles × 2 × 96,485 C/mol ≈ 19,700 C
Now, we can use the equation Q = I × t, where Q is the charge passed (in Coulombs), I is the current (in Amperes), and t is the time (in seconds).
Rearranging the equation to solve for time, we have:
t = Q / I
t = 19,700 C / 5 A
t ≈ 3,940 seconds
Therefore, the time taken for 6g of nickel to be deposited with a current of 5A is approximately 3,940 seconds.