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The charge required to liberate 11.5 g sodium from fused sodium chloride is
- a)0.5 Faraday
- b)1.0 Faraday
- c)1.5 Faraday
- d)96500 Coulomb
Correct answer is option 'A'. Can you explain this answer?
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The charge required to liberate 11.5 g sodium from fused sodium chlori...
To determine the charge required to liberate 11.5 g of sodium from fused sodium chloride, we can use Faraday's law of electrolysis.
Faraday's law states that the amount of substance liberated at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The relationship is given by the equation:
Q = nF
Where Q is the charge in coulombs, n is the number of moles of the substance being liberated, and F is the Faraday constant.
We can start by calculating the number of moles of sodium in 11.5 g. The molar mass of sodium is 22.99 g/mol, so:
Moles of sodium = mass of sodium / molar mass of sodium = 11.5 g / 22.99 g/mol ≈ 0.5 mol
Now we can calculate the charge required using Faraday's law:
Q = nF = 0.5 mol * F
To find the value of F, we need to know the charge on one mole of electrons. This is equal to the Avogadro constant (6.022 x 10^23) times the charge of one electron (1.602 x 10^-19 C):
Charge on one mole of electrons = Avogadro constant * charge of one electron ≈ 6.022 x 10^23 * 1.602 x 10^-19 C ≈ 96500 C
Therefore, the charge required to liberate 11.5 g of sodium from fused sodium chloride is approximately 0.5 * 96500 C = 48250 C, which is equivalent to 0.5 Faraday.
Hence, the correct answer is option A) 0.5 Faraday.
Faraday's law states that the amount of substance liberated at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The relationship is given by the equation:
Q = nF
Where Q is the charge in coulombs, n is the number of moles of the substance being liberated, and F is the Faraday constant.
We can start by calculating the number of moles of sodium in 11.5 g. The molar mass of sodium is 22.99 g/mol, so:
Moles of sodium = mass of sodium / molar mass of sodium = 11.5 g / 22.99 g/mol ≈ 0.5 mol
Now we can calculate the charge required using Faraday's law:
Q = nF = 0.5 mol * F
To find the value of F, we need to know the charge on one mole of electrons. This is equal to the Avogadro constant (6.022 x 10^23) times the charge of one electron (1.602 x 10^-19 C):
Charge on one mole of electrons = Avogadro constant * charge of one electron ≈ 6.022 x 10^23 * 1.602 x 10^-19 C ≈ 96500 C
Therefore, the charge required to liberate 11.5 g of sodium from fused sodium chloride is approximately 0.5 * 96500 C = 48250 C, which is equivalent to 0.5 Faraday.
Hence, the correct answer is option A) 0.5 Faraday.
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The charge required to liberate 11.5 g sodium from fused sodium chlori...
Use Farady's first law to get the answer..
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